How much energy is required to vaporize 98.6 g of ethanol (c2h5oh) at its boiling point, if its δhvap is 40.5 kj/mol? how much energy is required to vaporize 98.6 g of ethanol (c2h5oh) at its boiling point, if its δhvap is 40.5 kj/mol? 52.8 kj 11.5 kj 86.7 kj 39.9 kj 18.9 kj

The amount of energy required will be 86.7 kJ.

Explanation:

Mass of ethanol = 98.6 g

Moles of ethanol =

Enthalpy of vaporization of ethanol =

To vaporize 1 mol of ethanol we need 40.5 kJ of energy.

Then for 2.1434 moles the energy required will be:

The closest answer from the given options is 86.7 kJ.

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