A gaseous mixture of O2 and N2 contains 35.4 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure

0 thoughts on “A gaseous mixture of O2 and N2 contains 35.4 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure”

1. Answer:

   0.565 atm

   Explanation:

   Let’s assume we have 100 g of the gas. We’d then have 35.4 g of N₂ and (100 – 35.4) 64.6 g of O₂.

   Now we convert those masses into moles, using their respective molar masses:

   • 35.4 g N₂ ÷ 28 g/mol = 1.26 mol N₂

   • 64.6 g O₂ ÷ 32 g/mol = 2.02 mol O₂

   Then we calculate the molar fraction of O₂:

   • Molar Fraction O₂ = [tex]\frac{2.02mol}{1.26mol+2.02mol}[/tex] = 0.616

   Finally we calculate the partial pressure of O₂:

   • Partial P = Total P * Molar Fraction = 0.565 atm

   Reply