Section 11.3

Gas Laws – simple mathematical relationships between the volume, temperature, pressure, and quantity of gas.

Pressure – the force per unit area on a surface

force

Pressure = area

Newton (N) – SI unit for force – 1 kg mass by 1 meter per second that is applied

Barometer measures pressure.

Units of Pressure – mm Hg (millimeters of Mercury) Average atm pressure at sea level and 0 Celsius is 760 mm Hg.

1 atm = 760 mm Hg = 760 torr

STP (standard temperature and pressure) 1 atm pressure and o degrees Celsius

Boyle’s Law – the volume of a fixed mass of gas varies inversely with the pressure at constant temp.

(formula)

Charles’ Law – the volume of a fixed mass of gas varies directly with the Kelvin temperature at constant pressure.

(formula)

Gay-Lussac’s law – pressure of a fixed mass of gas varies directly with the Kelvin temperature at constant volume.

(formula)

Combined Gas Law – expresses the relationship between pressure, volume, and temperature of a gas when the amount of gas is fixed.

(formula)

Dalton’s Law of Partial Pressure: the total pressure of a mixture of gases is equal to the sum of the partial pressures of the ocmponent gases.

(formula)