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22 February, 08:11

The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 torr, respectively, at 296 K. What is the vapor pressure of a solution containing 50.0 g of each compound

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  1. 22 February, 09:37
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    273.84 Torr

    Given

    Carbon disulfide = CS2

    Carbon tetrachloride = CCL4

    CS2 Partial Pressure = 360 Torr

    CCL4 Partial Pressure = 99.8 Torr

    Grams of CS2 and CCL4 = 50g each

    Molar Mass of CS2 = 76.139 g/mol

    Molar Mass of CCL4 = 153.82 g/mol

    Calculating Moles of both substance ...

    The molar fraction is calculated by dividing the grams by the molar mass to get moles of each substance

    Moles of CS2 = 50g/76.139g/mol

    = 0.6567 mol

    Moles of CCL4 = 50g/153.82g/mol

    = 0.3251 mol

    Total = 0.6567 + 0.3251 = 0.9818

    Then, we find the Mole fraction of each substance.

    Mole Fraction of CS2 = 0.6567/0.9818

    = 0.6689

    Mole fraction CCL4 = 0.3251/0.9818

    = 0.3311

    Vapour Pressure of Solution is calculated by

    Mole fraction CS2 * Partial pressure CS2 + Mole fraction CCL4 * Partial pressure CCL4

    Vapour Pressure = 0.6689 * 360 + 0.3311 * 99.8

    = 240.80 + 33.04

    = 273.84 Torr

    = atm
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