At a certain temperature the vapor pressure of pure chloroform (CHCl3) is measured to be 91. torr. Suppose a solution is prepared by mixing

Question

At a certain temperature the vapor pressure of pure chloroform (CHCl3) is measured to be 91. torr. Suppose a solution is prepared by mixing 140. g of chloroform and 67.1 g of heptane (C,H16) of chloroform and 67.1 g of heptane (C7H16 Calculate the partial pressure of chloroform vapor above this solution.

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2 weeks 2021-07-22T21:19:24+00:00 1 Answers 5 views 0

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    2021-07-22T21:20:38+00:00

    Answer:

    P_{CCl_4}=52.43torr

    Explanation:

    Hello there!

    In this case, sine the solution of this problem require the application of the Raoult’s law, assuming heptane is a nonvolatile solute, so we can write:

    P_{CCl_4}=x_{CCl_4}P_{CCl_4}^{vap}

    Thus, we first calculate the mole fraction of chloroform, by using the given masses and molar masses as shown below:

    x_{CCl_4}=\frac{140/153.81}{140/153.81+67.1/100.21}=0.576

    Therefore, the partial pressure of chloroform turns out to be:

    P_{CCl_4}=0.576*91torr\\\\P_{CCl_4}=52.43torr

    Regards!

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