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Ch.11 - Liquids, Solids & Intermolecular Forces
Chapter 11, Problem 58

A 100.0-mL sample of water is heated to its boiling point. How much heat (in kJ) is required to vaporize it? (Assume a density of 1.00 g/mL.)

Verified step by step guidance
1
Calculate the mass of the water sample using the given density: mass=volume×density.
Use the mass of water to find the number of moles: moles=massmolar mass of water.
Determine the heat of vaporization for water, which is typically given as 40.7 kJ/mol.
Calculate the total heat required to vaporize the water using the formula: heat=moles×heat of vaporization.
Express the final answer in kilojoules (kJ).