The vapor pressure of pure carbon tetrachloride, CCl4, (molar
mass 153.82 g/mol) is 0.354 atm, and the vapor pressure of pure
chloroform, CHCl3 (molar mass 119.38 g/mol), is 0.526 atm at 316 K.
A solution is prepared from equal masses of the two compounds at
this temperature. If the vapor over the original solution is
condensed and isolated into a separate flask, what with the vapor
pressure of the chloroform be above this new solution?