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8 January, 21:44

At a certain temperature, a mixture of 2 gases, 11.2 g of oxygen and 104.75 of krypton exert a total pressure of 4.25 atm. What is the partial pressure of each gas in mm Hg?

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  1. 8 January, 21:55
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    Pressure of O₂ = 0.93 atm

    Pressure of krypton = 3.32 atm

    Explanation:

    This problem can be solved by using Dalton's Law of Partial Pressures, which states that the partial pressure of a component of a gaseous mixture depends on the mole ratio of said component and the total pressure of the gaseous mixture.

    Pₐ = Xₐ * Ptotal

    P ₐ - the partial pressure of component a

    χ ₐ - its mole fraction in the mixture

    P total - the total pressure of the mixture

    The moles of the two gases are:

    moles of O₂ = 11.2/32 = 0.35 moles

    moles of krypton = 104.75/83.8 = 1.25 moles

    Total moles = 1.25 + 0.35 = 1.6 moles

    Xₐ = number of moles of a / total moles in mixture

    Pressure of O₂ = 0.35/1.6 * 4.25 = 0.93 moles

    Pressure of krypton = 1.25/1.6 * 4.25 = 3.32 moles
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