In: Chemistry
The boiling point of pure ethanol at 760. torr is 82.0 degrees celsius. What would bet the vapor pressure of ethanol over a solution containing 2.13 mole of nonvolatile hydrocarbon and 15.30 moles of ethanol at 85.9 degrees celsius?
Solution :-
formula to calculate the vapor pressure of the solution is as follows
Vapor pressure of solution = mole fraction of solvent * vapor pressure of pure solvent
lets first calculate the mole fraction of the ethanol
mole fraction of ethanol = moles of ethanol / total moles
= 15.30 mol / (15.30 mol + 2.13 mol )
= 0.8778
now lets calculate the vapor pressure of the solution
Vapor pressure of solution = mole fraction of solvent * vapor pressure of pure solvent
= 0.8778 * 760 torr
= 667 torr
Therefore vapor pressure of the solution = 667 torr