Introduction to heat and energyby I CHOLOSI

Matter

bull Everything is made of MATTERbull Matter is anything that has volume and mass

bull Volume is the amount of space an object takes up or

occupies

It is easier to open a tight bottle cap by exposing it to

heat

It is easier to open a tight bottle cap by exposing it to

heat

THERMAL EXPANSIONTHERMAL EXPANSION

EXPANSION OF MATERIALSEXPANSION OF MATERIALS

ldquoMaterials expand as their thermal energy increasesrdquo rarr Thermal expansion

EXPANSION OF

MATERIALS UNDER 100degC

EXPANSION OF

MATERIALS UNDER 100degC

Materials (1 m in length)

Length of Expansion

Invar (alloy of Fe and Ni) 01 mm

Pyrex 03 mm

Platinum alloy 09 mm

Glass 09 mm

Concrete 10 mm

Steel 10 mm

Brass 20 mm

Aluminum 30 mm

Materials contract as their thermal energy decreasesrdquo

Measuring the volume of liquids

bull Liquids have volume We measure that volume with a graduated cylinder

bullUse the markings to determine the sig figs

bullAlways measure at the bottom of the meniscus

bullA liquid in any container has a meniscusbullLiters (L) and mL (milliliters) are most often used to express the volume of liquids

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Matter

bull Everything is made of MATTERbull Matter is anything that has volume and mass

bull Volume is the amount of space an object takes up or

occupies

It is easier to open a tight bottle cap by exposing it to

heat

It is easier to open a tight bottle cap by exposing it to

heat

THERMAL EXPANSIONTHERMAL EXPANSION

EXPANSION OF MATERIALSEXPANSION OF MATERIALS

ldquoMaterials expand as their thermal energy increasesrdquo rarr Thermal expansion

EXPANSION OF

MATERIALS UNDER 100degC

EXPANSION OF

MATERIALS UNDER 100degC

Materials (1 m in length)

Length of Expansion

Invar (alloy of Fe and Ni) 01 mm

Pyrex 03 mm

Platinum alloy 09 mm

Glass 09 mm

Concrete 10 mm

Steel 10 mm

Brass 20 mm

Aluminum 30 mm

Materials contract as their thermal energy decreasesrdquo

Measuring the volume of liquids

bull Liquids have volume We measure that volume with a graduated cylinder

bullUse the markings to determine the sig figs

bullAlways measure at the bottom of the meniscus

bullA liquid in any container has a meniscusbullLiters (L) and mL (milliliters) are most often used to express the volume of liquids

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

It is easier to open a tight bottle cap by exposing it to

heat

It is easier to open a tight bottle cap by exposing it to

heat

THERMAL EXPANSIONTHERMAL EXPANSION

EXPANSION OF MATERIALSEXPANSION OF MATERIALS

ldquoMaterials expand as their thermal energy increasesrdquo rarr Thermal expansion

EXPANSION OF

MATERIALS UNDER 100degC

EXPANSION OF

MATERIALS UNDER 100degC

Materials (1 m in length)

Length of Expansion

Invar (alloy of Fe and Ni) 01 mm

Pyrex 03 mm

Platinum alloy 09 mm

Glass 09 mm

Concrete 10 mm

Steel 10 mm

Brass 20 mm

Aluminum 30 mm

Materials contract as their thermal energy decreasesrdquo

Measuring the volume of liquids

bull Liquids have volume We measure that volume with a graduated cylinder

bullUse the markings to determine the sig figs

bullAlways measure at the bottom of the meniscus

bullA liquid in any container has a meniscusbullLiters (L) and mL (milliliters) are most often used to express the volume of liquids

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

EXPANSION OF

MATERIALS UNDER 100degC

EXPANSION OF

MATERIALS UNDER 100degC

Materials (1 m in length)

Length of Expansion

Invar (alloy of Fe and Ni) 01 mm

Pyrex 03 mm

Platinum alloy 09 mm

Glass 09 mm

Concrete 10 mm

Steel 10 mm

Brass 20 mm

Aluminum 30 mm

Materials contract as their thermal energy decreasesrdquo

Measuring the volume of liquids

bull Liquids have volume We measure that volume with a graduated cylinder

bullUse the markings to determine the sig figs

bullAlways measure at the bottom of the meniscus

bullA liquid in any container has a meniscusbullLiters (L) and mL (milliliters) are most often used to express the volume of liquids

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Measuring the volume of liquids

bull Liquids have volume We measure that volume with a graduated cylinder

bullUse the markings to determine the sig figs

bullAlways measure at the bottom of the meniscus

bullA liquid in any container has a meniscusbullLiters (L) and mL (milliliters) are most often used to express the volume of liquids

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Physical Changes

A physical change is a change that affects one or more physical properties of a substance

Physical changes do not form new substances EX ice melting or sugar dissolving

Physical changes are easy to undo

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Chemical Changes

A chemical change occurs when one or more substances are changed into entirely new substances with different properties

bull You can observe chemical properties only when a chemical change might occur

Examples of chemical changes baking a cake

bullrusting

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Heat in the city

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

MEASURING TEMPERATUREMEASURING TEMPERATURE

1 Using the tactile sense1 Using the tactile sense

2 Using a thermometer2 Using a thermometer

a Thermal sensora Thermal sensor

b Calibrations ~ degF degC or Kb Calibrations ~ degF degC or K

PARTS OF A THERMOMETER

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

TYPES OF THERMOMETERTYPES OF THERMOMETER1

Dia

l the

rmom

eter

ndash a

ka R

otar

y th

erm

omet

er

2 Glass thermometer ndash aka

liquid-in-glass ~ Mercury or

Colored alcohol

3

Ther

moc

oupl

e

ndash ak

a el

ectr

onic

th

erm

omet

er

4 Liquid crystal thermometer4 Liquid crystal thermometer

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

TEMPERATURE SCALESTEMPERATURE SCALES

2 Celsius Scale ndash (named after Swed astronomer Anders C Celsius) based on the freezing and boiling point of water at normal atmospheric pressure ~ 0ordmC - freezing pt and 100ordmC ndash boiling pt

Fahrenheit Scale ndash (named after Ger physicist Gabriel Daniel Fahrenheit) based on the freezing and boiling point of water at normal atmospheric pressure ~ 32ordmF - freezing pt and 212ordmF ndash boiling point

Kelvin Scale ndash (named after Brit physicist William T Kelvin) erased the arbitrary assigned reference points thus called not a relative scale but an Absolute temperature scale 0 = nothing ndash Absolute Zero ~ lowest temperature possible occurring when all random motion of molecules has ceased In this scale 273K ndash freezing pt of water 373K ndash boiling pt

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

CONVERSIONSCONVERSIONS

(degF -32)59From degF to degC

From degC to degF (degC 95) + 32

From degC to K degC + 273

From degF to K (degF-32)59 + 273

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Detailed information about temperature scale

Temperature Scales -Fahrenheit

Celsius

Kelvin

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Fahrenheit Scale

bull Develop in early 1700s by G David Fahrenheit

bull Zero is the lowest temperature that salt water will freeze

bull 32deg F is freezing point of pure water

bull 212deg F is boiling point of pure water

bull F scale used in US for surface temperatures

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

bull Developed in 1700s

bull Also called Centigrade scale

bull Zero is the freezing point of pure water

bull 100 is the boiling point of pure water at sea

level

bull A change of 1 Cdeg = 18Fdeg

bull 18 C = F -32

Celsius Scale

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

bull Absolute zero ndash molecules stop moving

bull Lowest possible temperatures

bull Zero K = -459deg F

bull Zero K = -273deg C

bull degK = degC + 273

bull Kelvin scale used for all scientific equations

Kelvin Scale

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Specific heat of common materials

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Temperature effects

A material with a high specific heat

can absorb a great deal of

thermal energy without a great

change in temperature

To calculate thermal energy changes in an object use the

following formula

Change in energy= mass X specific heat X change in temperature

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Example

bull How much heat is needed to raise the temperature of 5 kilograms of water by 10 kelvins

Change in energy= mass X specific heat X change in temperature=5 kg X 4180 J(kg X K) X 10 K= 209000 J

You need to transfer 209000 joules to the water to increase its temperature by 10 kelvins

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

THERMOSTAT

ldquordquo The amount of expansion of a material depends on the change

in temperature

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

This is it

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

The study of the flow of heat within an object or from one medium to another due to their variation in temperature

HEAT TRANSFER

Radiation - energy is emitted in the form of electromagnetic waves or subatomic particles eg bull heatwarmth felt from a flame or bonfire sans touching it the heat from the

microwave oven and the heat from the sunbull 2 Conduction - heat energy transfer caused by direct contact wherein heat travels

from one molecule to another For example exposing metal to a flame allowing an article to rest on a warm or hot object

bull 3 Convection - transference of mass or heat within a fluid caused by the tendency of warmer and less dense material to rise producing air or fluid currents

METHODS OF HEAT

TRANSFER

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Drinking coffee

Conduction

Radiation

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

ldquoHeat flows from a region of high concentration to a region of low

concentrationrdquo

Hot rarr ColdHot rarr Cold

LegendLegend

Hot air risesHot air rises Air cools down

becomes dense

Air cools down

becomes dense

Cold air sinksCold air sinksAir heats up and

becomes less dense

Air heats up and becomes less

dense

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

SPECIFIC HEATSPECIFIC HEAT

The amount of energy required to raise the temperature of one kilogram (1 kg) of a substance by one degC (1degC) or one Kelvin (1 K) It is expressed in terms of Joules per kilogram-Kelvin (JkgmiddotK) or Joules per kilogram degree Celsius (JkgmiddotdegC) or calorie per gram degree Celcius (calgmiddotdegC) in which 1 cal = 4186 J

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

THERMAL CAPACITYTHERMAL CAPACITY

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

The amount of heat required to raise the temperature of a substance by 1 degree (1deg) and is the product of its mass and specific heat

ΔQ = mCΔTΔQ = mCΔTWherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Wherein ΔQ is change in heat expressed in terms of Jm is the mass of the substance in kgC is the specific heat in JkgmiddotKΔT is the change in heat in K

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Heat Transfer Song

bull httpwwwyoutubecomwatchv=wr8Z4SCETPshttpwwwyoutubecomwatchv=wr8Z4SCETPs

httpwwwglogstercomderp54examples-of-energy-transformationsg-6lgnaq3gr48lgm8rkn52ua0

Energy is always being transferred between objects are different temperatures

bull It is often important to slow this movement of energy

bullThink-Pair-Share Think of one situation where it would be important to slow the movement of energy

Different Materials Are Used to Control the Transfer of Energy

HttpgooglOQau2p

httpgooglIaw4Kd

httpgooglImRnRa

httpgooglglKX2e

httpgooglNRBmyS

These slides have been repurposed from

HttpgooglOQau2p

httpgooglIaw4Kd

httpgooglImRnRa

httpgooglglKX2e

httpgooglNRBmyS

These slides have been repurposed from