In: Chemistry
What is the vapor pressure of an ideal solution of ethanol if 1 mile of glycerin is placed in 4 moles of ethanol at 40?C? Pure ethanol has a vapor pressure of 135.3 torr.
Solution :-
Vapor pressure of solution = mole fraction of solvent * vapore pressure of pure solvent
lets calculate the mole fraction of the ethanol
mole fraction of ethnaol = moles of ethanol / total moles
= 4 mol / (4 mol + 1 mol )
= 0.8
Vapor pressure of solution = mole fraction of solvent * vapore pressure of pure solvent
= 0.8 * 135.3 torr
= 108.24 torr
Therefore vapore pressure of solution = 108.24 torr