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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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sebassandin

Answer:

[tex]P_{CCl_4}=52.43torr[/tex]

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:

[tex]P_{CCl_4}=x_{CCl_4}P_{CCl_4}^{vap}[/tex]

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

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

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

[tex]P_{CCl_4}=0.576*91torr\\\\P_{CCl_4}=52.43torr[/tex]

Regards!

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