A solution is made by mixing \(50.0 \mathrm{~g}\) of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}ight)\) and \(50.0 \mathrm{~g}\) of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}ight)\). What is the vapor pressure of this solution at \(25^{\circ} \mathrm{C}\) ? What is the composition of the vapor expressed as a mole fraction? Assume ideal solution and gas behavior. (At \(25^{\circ} \mathrm{C}\) the vapor pressures of pure acetone and pure methanol are 271 and 143 torr, respectively.) The actual vapor pressure of this solution is 161 torr. Explain any discrepancies.