Kinetic Theory

•All matter is made up of tiny particles

•The particles are in constant motion

•All collisions are elastic

Pressure

•Force per unit area

•Caused by collisions against a surface

•Gas measured in pressure

Units of Pressure•kPa: kilopascal (Std Unit)

•Pascal: newton/sq. meter

•Atmosphere (Atm):

•mm Hg:

Standard Pressure•101.3 kPa (to be changed)•1.00 Atm•760 mm Hg or Torrs•30.0 inches Hg•1013 millibars

Gas Laws

State the Following Laws

• Boyle’s Law

• Charles’ Law

• Gay Lussac’s Law

• Dalton’s Law

• Graham’s Law

Boyle’s Law

•The pressure & volume of a gas at constant

temperature are inversely proportioned

P1V1 = P2V2 = K

Charles’ Law

• The volume and temperature of a gas at constant pressure

are directly proportioned

V1 V2

T1 T2

= = K

Guy Lussac’s

Law

• The pressure and temp. of a gas at constant volume are

directly proportioned

P1 P2

T1 T2

= = K

Combined Gas Law

•Combination of the three formulas

P1V1 P2V2

T1 T2

=

Common Sense

•A gas’s volume is directly proportioned to its number

of moles

V1 V2

n1 n2

= = K

New Combination

P1V1/n1T1 =

P2V2/n2T2 = K

New Combination

P1V1 P2V2

n1 T1 n2T2

= = K

Ideal Gas Law

PV = nRT

Dalton’s Law

•The total pressure = the sum of the partial pressures

PT = P1 + P2 + etc

Graham’s Law

• The velocities of particles are inversely proportioned to the square root of their masses

v1 M2

v2 M1

=

Calculate the new volume of 5.0 L of

gas when its pressure is doubled and its

temperature is tripled:

Calculate the volume of a gas at STP when it occupied 150.0 mL

at 227oC under303.9 kPa pressure:

Calculate the volume of 3.0 moles of gas at

-23oC under 83.1 kPa pressure.

Calculate the number of moles of gas occupying 831 mL under 250 kPa

at 227oC.

Calculate the ratio of the

velocities of He gas to HCl gas:

Calculate the mass of CO2 occupying 83.1 L under 25 GPa at

227oC

Calculate the molecular mass of 5.0

g of gas occupying 831L under 250

MPa at 227oC

Calculate the density of carbon dioxide at 27oC under 83.1 kPa

pressure

Integrated Formulas

Ideal Gas Law

PV = nRT

Related Formulasm

V

m/n

D or =

M =

M = m/n

n = m/MPV = nRT

mRT

MmRT

PV

PV =

M =

m

V

mRT

PV

D =

M =

m

V

m RT

V P

D =

M =

DRT

P

M P

RT

M =

D =

The total pressure of a system is 120.0 kPa.

The partial pressure of gas A is 112.0 kPa.

Determine the pressure of gas B

Calculate the mass of 831 mL of CO2 at 27oC under 150 kPa

pressure:

Calculate the volume of a gas at STP when it occupies 80.0 mL at 127oC under 303.9 kPa

pressure:

5 Calculate the volume of 4.0 moles of gas

under 83.1 kPa pressure at 127oC:

Calculate the molecular mass of 50 g of gas occupying 831L under 250

MPa at 227oC

Calculate the mass of 831 mL of CO2 at 167oC under 150 kPa

pressure:

The total pressure of a system is 120.0 kPa.

The partial pressure of gas A is 112.0 kPa.

Determine the pressure of gas B

The total pressure of a system is 150.0 kPa. The system contains 50 % A,

30 % B, & 20 % C. Determine the pressure

of each gas.

Calculate the density of carbon dioxide at 27oC under 83.1 kPa

pressure

Calculate the velocity HBr

when the velocity Be is 270 m/s:

Calculate the final volume that 3.0 L of gas

will obtain when the absolute temperature is tripled & the pressure is

halved.

Calculate the mass of CO occupying 831 kL at 227oC under 2.50 Mpa

pressure.

Calculate the volume of H2 formed at 27oC

under 150 kPawhen 6.8 mg NH3

decomposes making N2 & H2.