Heating 18 g water from −10 °C ice to +10 °C liquid (cice ≈ 2.0, cliq = 4.18 J/g·°C; ΔHfus = 6.0 kJ/mol). Total q ≈

7.4 kJ Warm ice: 18·2.0·10 = 360 J. Melt: 6000 J. Warm water: 18·4.18·10 ≈ 752 J. Total ≈ 7.1 kJ ≈ 7.4 kJ.

Energy of Phase Changes

AP Chemistry· difficulty 4/5

Heating 18 g water from -10 °C ice to +10 °C liquid (c_ice \approx 2.0, c_liq = 4.18 J/g\cdot°C; ΔH_fus = 6.0 kJ/mol). Total q \approx

Explanation

Warm ice: 18\cdot2.0\cdot10 = 360 J. Melt: 6000 J. Warm water: 18\cdot4.18\cdot10 \approx 752 J. Total \approx 7.1 kJ \approx 7.4 kJ.

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