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30 May, 17:46

At a given temperature, the vapor pressure of pure acetone (CH3COCH3, 58.00 g/mol) is 342 torr. At the same temperature, the vapor pressure of pure chloroform (CHCl3, 119.35 g/mol) is 230 torr. Consider a solution containing 23.2 g of acetone and 73.8 g of chloroform. Calculate the total vapor pressure above the solution (in torr to 0 decimal places)

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  1. 30 May, 17:48
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    Total vapor pressure = 274 torr

    Explanation:

    According to Raoult's law, the partial pressure of a volatile compound in a mixture of two volatile components is

    PA = Xa PºA where PA = partial pressure of component A

    XA = mole fraction of A = mol A / (molA + Mol B)

    PºA = vapor pressure of pure A

    and the total pressure will be given by the sum of the partial pressures.

    mol CH3COCH3 = 23.2 g / 58 g/mol = 0.40 mol

    mol CHCl3 = 73.8 g / 119.35 g/mol = 0.62 mol

    total mol = 0.40 mol + 0.62 mol = 1.02 mol

    XCH3COCH3 = 0.40 mol / 1.02 mol = 0.39

    XCHCl3 = 0.62 mol / 1.02 mol = 0.61

    PCH3COCH3 = 0.39 x 342 torr = 133.4 torr

    PCHCl3 = 0.61 x 230 torr = 140.3 torr

    Ptotal = 133.4 torr + 140.3 torr = 274 torr
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