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.)

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1. <Calculate the mass of the water sample using the given density: \( \text{mass} = \text{volume} \times \text{density} \).>
2. <Use the mass of water to find the number of moles: \( \text{moles} = \frac{\text{mass}}{\text{molar mass of water}} \).>
3. <Determine the heat of vaporization for water, which is typically given as \( 40.7 \text{ kJ/mol} \).>
4. <Calculate the total heat required to vaporize the water using the formula: \( \text{heat} = \text{moles} \times \text{heat of vaporization} \).>
5. <Express the final answer in kilojoules (kJ).>