A solution is made by dissolving 13.75 mol of non-volatile solute into 34.15 mol of solvent. If the vapor pressure of the pure solvent at room temperature is 48.60 torr, what will be the vapor pressure (in torr) of the solution described at the same temperature?
Answer
34.65 torr
Explanation
According to Roult's law
Psolution = XsolventP°solvent
where,
Psolutionn= Vapor pressure of solution
Xsolvent = mole fraction of solvent
P°solvent = vapor pressure of solvent in its pure state. 48.60torr
Mole fraction = number of moles / Total number of moles
number of moles of solute = 13.75mol
number of moles of solvent = 34.15
Total number of moles = 47.90mol
mole fraction of solvent = 34.15mol/ 47.90mol = 0.7129mol
Psolution = 0.7129 × 48.60torr
Psolution = 34.65 torr
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