Question

What is the partial pressure of hydrogen gas in a mixture that contains 6.00 grams of hydrogen gas and 1.80 mol carbon dioxide with a total pressure of 12.0 atm?

Answer 1

Answer:

P(H₂ ) =  7.5 atm

Explanation:

Given data:

Mass of hydrogen = 6.00 g

Number of moles of CO₂ = 1.80 mol

Total pressure = 12.0 atm

Partial pressure of H₂ = ?

Solution:

Number of moles of H₂:

Number of moles = mass/molar mass

Number of moles = 6.00 g/ 2 g/mol

Number of moles = 3 mol

Partial pressure of gases:

Total number of moles present = 1.80 mol + 3 mol = 4.80 mol

P(H₂ ) = [ 3 mol/ 4.80 mol] × 12.0 atm

P(H₂ ) = 0.625× 12.0 atm

P(H₂ ) =  7.5 atm

P(CO₂) = [1.80 mol/4.80 mol] × 12.0 atm

P(CO₂) = 0.375 × 12.0 atm

P(CO₂) = 4.5 atm