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8 December, 00:53

A solution is prepared by mixing 0.0300 mol CH2Cl2 and 0.0500 mol CH2Br2 at 25 degrees C. Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions) at 25 degrees C. At 25 degrees C, the vapor pressures of pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively.

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  1. 8 December, 02:47
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    CH2Cl2 mole fraction = 0.833

    CH2Br2 mole fraction = 0.167

    Explanation:

    Step 1: Data given

    Number of moles CH2Cl2 = 0.0300 moles

    Number of moles CH2Br2 = 0.0500 moles

    Temperature = 25 °C

    Vapor pressure of pure CH2Cl2 = 133 torr

    Vapor pressure of pure CH2Br2 = 11.4 torr

    Step 2: Calculate mol fraction in solution

    Mol fraction CH2Cl2 = 0.0300 moles / (0.0300 + 0.0700)

    Mol fraction CH2Cl2 = 0.300

    Mol fraction CH2Br2 = 0.0700 moles / (0.0300 + 0.0700)

    Mol fraction CH2Br2 = 0.700

    Step 3: Calculate partial pressure

    Partial pressure CH2Cl2 = 133 torr * 0.300 = 39.9 torr

    Partial pressure CH2Br = 11.4 torr * 0.700 = 7.98 torr

    Step 4: Calculate the total pressure

    total pressure = 39.9 + 7.98 = 47.88 torr

    Step 5: Calculate mol fraction

    partial pressure / total pressure = mole fraction

    CH2Cl2 mole fraction = 39.9 / 47.88 = 0.833

    CH2Br2 mole fraction = 7.98 / 47.88 = 0.167
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