34.5k views
7 votes
16.A mixture of carbon dioxide and hydrogen gases contains carbon dioxide at a partial pressure of 217 mm Hg and hydrogen at a partial pressure of 703 mm Hg. What is the mole fraction of each gas in the mixture?

XCO2 =

XH2 =

User ZeroDefect
by
2.8k points

1 Answer

10 votes

x CO₂ = 0.236

x H₂ = 0.764

Further explanation

Given

P CO₂ = 217 mmHg

P H₂ = 703 mmHg

Required

The mole fraction

Solution

Dalton's law :

The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

Can be formulated:

P tot = P1 + P2 + P3 ....

P tot for the mixture :

= 217 mmHg + 703 mmHg

= 920 mmHg

Mole fraction of each gas :

x CO₂ = 217 mmHg/920 mmHg = 0.236

x H₂ = 703 mmHg/920 mmHg = 0.764

User Raedawn
by
3.0k points