How many grams of CO2 gas would occupy 33.7 L of volume at a temperature of

-22.2oC and a pressure of 990 mm Hg?

93.75 g.

Explanation:

Firstly, we need to calculate the no. of moles of a gas, we can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm (P = 990 mmHg = 1.3 atm).

V is the volume of the gas in L (33.7 L).

n is the no. of moles of the gas in mol.

R is the general gas constant (R = 0.082 L. atm/mol. K),

T is the temperature of the gas in K (T = - 22.2°C + 273 = 250.8 K).

∴ n = PV/RT = (1.3 atm) (33.7 L) / (0.082 L. atm/mol. K) (250.8 K) = 2.13 mol.

The no. of grams of CO₂ = no. of moles x molar mass = (2.13 mol) (44.01 g/mol) = 93.75 g.