A solution contains 0.0442 mol of ethanol and 0.715 mol of waterat 25 oC. The vapor pressures of pure ethanol and pure water at 25oC are 44.6 torr and 23.8 Torr, respectively.
a) Assuming ideal behavior, calculate the total vapor pressureabove the solution.
b) If the actual vapor pressure above the solution is found tobe 28.3 Torr, is the solution behaving ideally? If not, whatinteractions are favored (the solute-solute and solvent-solventinteractions, or the solute interactions)?
