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29 November, 00:03

A mixture of krypton and argon gases, at a total pressure of 733 mm Hg, contains 3.97 grams of krypton and 6.34 grams of argon. What is the partial pressure of each gas in the mixture?

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  1. 29 November, 00:12
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    Partial pressure of krypton = 167.12 mmHg

    Partial pressure of argon = 565.88 mmHg

    Explanation:

    The partial pressure of a gas in a mixture of gasses is equal to the total pressure multiplied (Pt) by the mole fraction of the gas (X):

    P = X Pt

    The total pressure is Pt = 733 mmHg

    The mole fraction is given by the following:

    X = number of moles of gas / total number of moles

    For krypton (Kr), the molecular weight is 83.8 g/mol and we calculate the number of moles by dividing the mass into the molecular weight as follows:

    moles of Kr = 3.97 g / (83.8 g/mol) = 0.047 moles

    For argon (Ar), the molesular weight is 39.9 g/mol, so we calculate the number of moles as follows:

    moles of Ar = 6.34 g / (39.9 g/mol) = 0.159

    Now, we calculate the total number of moles (nt):

    nt = moles of Kr + moles of Ar = 0.047 moles + 0.159 moles = 0.206 moles

    The mole fraction of each gas is now calculated:

    X (Kr) = moles of Kr/nt = 0.047 moles/0.206 = 0.228

    X (Ar) = moles of Ar/nt = 0.159 moles/0.206 = 0.772

    Finally, with the mole fractions and the total pressure we calculate the partial pressure of each gas as follows:

    P (Kr) = X (Kr) x Pt = 0.228 x 733 mmHg = 167.12 mmHg

    P (Ar) = X (Ar) x Pt = 0.772 x 733 mmHg = 565.88 mmHg
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