Question Solved1 Answer 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.)

GIERCY The Asker · Chemistry

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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Step 1Density of water = 1.00 g/mLVolume of water = 100 mLHeat of vaporization of water = 40.7 kJ/molMass of water = density × volume                            = 1.00 g/mL &#21 ... See the full answer