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Thermochemistry
THERMODYNAMICS
Courtesy of lab-initio.com
Ch 17 textbook
Get out your notes and your calculator.
Thermochemistry
First Law of Thermodynamics
• Energy is neither created nor destroyed.
• In other words, the total energy of the universe is a constant; if the system loses energy, it must be gained by the surroundings, and vice versa.
Thermochemistry
Changes in Internal Energy
• When energy is exchanged between the system and the surroundings, it is exchanged as either heat (q) or work (w).
• That is, E = q + w.
Thermochemistry
Calorimetry The amount of heat absorbed or released during a
physical or chemical change can be measured,
usually by the change in temperature of a known
quantity of water in a calorimeter.
Thermochemistry
Heat Capacity and Specific Heat
• The amount of energy required to raise the temperature of a substance by 1 K (1C) is its heat capacity.
• We define specific heat capacity (or simply specific heat) as the amount of energy required to raise the temperature of 1 g of a substance by 1 K.
Thermochemistry
Specific Heat
Substance Specific Heat (J/g·K)
Water (liquid) 4.18
Ethanol (liquid) 2.44
Water (solid) 2.06
Water (vapor) 1.87
Aluminum (solid) 0.897
Carbon (graphite,solid) 0.709
Iron (solid) 0.449
Copper (solid) 0.385
Mercury (liquid) 0.140
Lead (solid) 0.129
Gold (solid) 0.129
The amount of heat required to raise the temperature of
one gram of substance by one degree Celsius.
Thermochemistry
Calculations Involving Specific Heat
c = Specific Heat Capacity
q = Heat lost or gained
T = Temperature change
𝑞 = 𝑐 × 𝑚 × ∆𝑇
m = mass
Thermochemistry
Calculate the amount of heat lost or gained by a
3.46 g sample of aluminum when the
temperature raises from 25.0°C to 45°C.
(Specific heat of aluminum = 0.902 J/g•°C) Is
this endothermic or exothermic? Why?
Thermochemistry
Calculate the amount of heat lost or gained by a
3.46 g sample of aluminum when the
temperature raises from 25.0°C to 45°C.
(Specific heat of aluminum = 0.902 J/g•°C) Is
this endothermic or exothermic? Why?
Thermochemistry
Determine the heat transferred from a piece of
metal heated to 85.0C when it is placed in a
coffee cup calorimeter with 150.0 g of water
initially at 22.5C and equilibrates with the water
at 32.1C.
If the piece of metal had a mass of 157.52g, then
what was the specific heat of the metal?
Thermochemistry
Determine the heat transferred from a piece of
metal heated to 85.0C when it is placed in a
coffee cup calorimeter with 150.0 g of water
initially at 22.5C and equilibrates with the water
at 32.1C.
If the piece of metal had a mass of 157.52g, then
what was the specific heat of the metal?
Thermochemistry
A 28.4 g sample of aluminum is heated
to 39.4 oC, then is placed in a
calorimeter containing 50.0 g of water.
Temperature of water increases from
21.00 oC to 23.00 oC. What is the
specific heat of aluminum?
Thermochemistry
A 28.4 g sample of aluminum is heated
to 39.4 oC, then is placed in a
calorimeter containing 50.0 g of water.
Temperature of water increases from
21.00 oC to 23.00 oC. What is the
specific heat of aluminum?