At 297 K the vapor pressure of pure carbon tetrachloride (CCl4) is 0.138 atm and the vapor pressure of pure chloroform (CHCl3) is 0.245 atm. Equal chemical amounts (equal numbers of moles) of carbon tetrachloride and chloroform are mixed and form an ideal solution. Compute the mole fraction of chloroform in the vapor in equilibrium with this solution. The mole fraction for both carbon tetrachloride and chloroform is 0.5, but when you find mole fraction of the vapor of chloroform you get 0.64? Doesn't this not follow the P_a/P_tot = n_a/n_tot equation?

Question

abb0t · Answer

Is this using Raoults Law? P = Pb + Pt = 1/2P...or something like that?

anonymous · Answer

yeah raoult;s law