The vapor pressure of carbon tetrachloride, CCl_4, is 0.354 atm and the vapor pr

Question

The vapor pressure of carbon tetrachloride, CCl_4, is 0.354 atm and the vapor pressure of chlcroofrm, CHCl_3, is 0.526 atm at 316 K.A solution is prepared from equal masses of these two compounds at this temperature. The mole fraction of chloroofrm in the vapor above this solution is X_CHCL_3 = 0.657. If the vapor above the original solution is condensed and isolated into a separate flask, the vapor pressure of chlcroofrm above this new solution is 0.346 atm. Calculate the mole fraction of chloroofrm in the vapor above a solution obtained by three successive separations and condensations of the vapors above the original solution of carbon detrachloride and chloroofrm. Show how this result explains the us of distillation as a separation method.

Explanation / Answer

Answer: According to the given informations , Here we have to used the formula PA = XA * Ptotal

Here Pa is partial pressure of A and Xa is mole fraction .

Now , using it for CHCl3 we get ,

0.526 = 0.657 * PTotal

Ptotal   = 0.80 atm

Hence mole fraction of CCl4 is

0.346 = XCCl4 * 0.80

Xccl4 = 0.4325

Hence the required answer is 0.4325 mole fraction of CCl4 . Thank you :)

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