The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two gases. What is the mole fraction of each gas in the mixture?

Question

The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two gases. What is the mole fraction of each gas in the mixture?

Answer 1

Dalton's law of partial pressures.

mole fraction of a gas x total pressure = partial pressure of the gas

partial pressure / total pressure = mole fraction

Total pressure = 0.175 atm + 0.250 atm = 0.425 atm

mole fraction CH₄ = 0.175 atm / 0.425 atm = 0.412

mole fraction O₂ = 0.250 atm / 0.425 atm = 0.588