Step-by-step explanation:

Relationship between Pressure- Volume (Boyle's Law)

•The volume of a fixed mass of gas at constant temperature is inversely proportional to the pressure exerted on it.

•P ∞ 1 / V then PV equals a constant value.

•Boyle’s Law:

P1V1 = P2V2 at constant temperature.

Relationship between Temperature- Volume (Charles' Law)

•The volume of a fixed mass of gas at constant pressure is directly proportional to its absolute temperature (kelvin scale).

•V ∞ T then V / T equals a constant value.

•Charles’ Law:

V1 = V2 at constant pressure

T1 T2

Relationship between Volume-Mole (Avogadro's Law)

Avogadro postulated that EQUAL volumes of gases at the same temperature and pressure CONTAIN equal numbers of particles.

V ∞ n or V= kn where k is a constant.

MOLAR gas Volume

•Molar Gas Volume is the volume of 1 mole of a particular gas.

•It has been found experimentally that 1 mole of any gas at STP occupies a volume of 22.7 L.

•The molar volume of a gas at SLC is 24.8 L.

•Gas constants:

VSTP = 22.7 L

VSLC = 24.8 L

STP- 0 oC and 100kPa

SLC – 25 oC and 100KPa

There is a direct relationship between the number of MOLES of a gas and its molar volume.

n = V

Vm

Where:

n is the number of moles of gas

V is the actual volume of gas

Vm is the molar volume of the gas

•Combine Boyle’s and Charles’ Laws:

PV equals a constant value

V / T equals a constant value

to get PV / T equals a constant value.

•Combined Gas Law:

P1V1 = P2V2 for a constant amount of gas.

T1 T2

•P ∞ 1 / V (Boyle’s Law)

•P ∞ T (Gay Lussac’s Law)

•P ∞ n

•Combine these proportionalities:

P ∞ nT / V

Universal gas equation

•Replace proportionality with equality sign.

•Introduce a general gas constant, R and we get the general gas equation.

PV = nRT

where:

Pressure (P) is measured in kilopascals (kPa)

Volume (V) is measured in litres (L)

Temperature (T) is measured in kelvin (K)

Number of moles (n) – unit (mol)

General Gas Constant (R) = 8.31JK-1mol