Question

A tank contains a mixture of 52.5g oxygen gas and 65.1g carbon dioxide gas at 27c. the total pressure in the tank is 9.21 atm calculate the partial pressure of each gas in the containter

Answer 1

The partial pressure of oxygen is 4.84 atm, and the partial pressure of carbon dioxide is 4.37 atm.

Moles of O₂ = 52.5 g O₂ × (1 mol O₂/32.00 g O₂) = 1.641 mol O₂

Moles of CO₂ = 65.1 g CO₂ × (1 mol CO₂/44.01 g CO₂) = 1.479 mol CO₂

Total moles = (1.641 + 1.479) mol = 3.120 mol

Let O₂ be Gas 1 and CO₂ be Gas 2.

χ₁= 1.641/3.120 = 0.5259

χ₂= 1.479/3.120 = 0.4741

p₁ = χ₁p_tot = 0.5259 × 9.21 atm = 4.84 atm

p₂ = χ₂p_tot = 0.4741 × 9.21 atm = 4.37 atm