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1 May, 09:55

A mixture of carbon dioxide and oxygen gases at a total pressure of 942 mm Hg contains carbon dioxide at a partial pressure of 720 mm Hg. If the gas mixture contains 11.6 grams of carbon dioxide, how many grams of oxygen are present?

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  1. 1 May, 10:16
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    2.6 g of O₂ are present in the mixture

    Explanation:

    The molar fraction concept to solve this:

    Partial pressure / Total pressure = Moles of a gas / Total moles in the mixture

    720 mmHg / 942 mmHg = 0.764

    This is the molar fraction of CO₂

    Sum of molar fraction in mixture = 1

    1 - 0.764 = 0.236

    This is molar fraction of O₂

    Molar mass CO₂ = 44.01 g/m

    Moles CO₂ = 11.6 g / 44.01 g/m → 0.263 moles

    Let's make the equation:

    0.236 = x / x + 0.263

    0.236 (x + 0.263) = x

    0.236x + 0.062 = x

    0.062 = x - 0.236x

    0.062 = 0.764x

    0.062 / 0.764 = x → 0.081

    These are the moles of O₂

    Moles. molar mass = mass

    0.081 m. 32g/m = 2.6 g
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