A solution of ethanol $($eth$)$ and chloroform $($chl$)$ at $45\backslash$deg C with Xeth $=0\mathrm{.}9900$ has a vapor pressure of $177\mathrm{.}95$ torr. At this high dilution of chloroform, the solution can be assumed to be essentially ideally dilute. The vapor pressure of pure ethanol at $45\backslash$deg C is $172\mathrm{.}76$ torr. $($a$)$ Find the partial pressures of the gases in equilibrium with the solution. $($b$)$ Find the mole fractions in the vapor phase. $($c$)$ Find the Henry's law constant for chloroform in ethanol at $45\backslash$deg C$.($d$)$ Predict the vapor pressure and vapor$-$phase mole fractions at $45\backslash$deg C for a chloroform$-$ethanol solution with Xeth $=0\mathrm{.}9800.$Compare with the experimental values P $=183\mathrm{.}38$ torr and X$"$eth $=0\mathrm{.}9242.$