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

Question

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 is 0.918 atm

in progress 0
Hồng Cúc 7 hours 2021-07-22T01:27:03+00:00 1 Answers 0 views 0

Answers ( )

    0
    2021-07-22T01:28:32+00:00

    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 = \frac{2.02mol}{1.26mol+2.02mol} = 0.616

    Finally we calculate the partial pressure of O₂:

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

Leave an answer

Browse

Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )