The boiling point of pure ethanol at 760. torr is 82.0 degrees celsius. What would bet...

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?

Expert Solution

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

queen_honey_blossom answered 2 years ago

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