Given that the heat of fusion of water is 6.02 kJ/mol, the heat capacity of H2O(l) is 75.2 J/mol·K, and the heat capacity of H2O(s) is 37.7 J/mol·K, calculate the total heat required to convert 1 mole of ice at -10°C to liquid water at 0°C.

• A. 5.52 kJ
• B. 6.52 kJ
• C. 7.02 kJ
• D. 6.02 kJ

Answer: (B)

Verified step by step guidance

1. Calculate the heat required to raise the temperature of ice from -10°C to 0°C using the formula q = m * C * ΔT, where m is the number of moles, C is the heat capacity of ice, and ΔT is the change in temperature.
2. Substitute the given values into the formula: m = 1 mol, C = 37.7 J/mol·K, and ΔT = 0°C - (-10°C) = 10 K.
3. Convert the calculated heat from joules to kilojoules by dividing by 1000, since 1 kJ = 1000 J.
4. Add the heat of fusion to the heat calculated in the previous step. The heat of fusion is the energy required to convert ice at 0°C to liquid water at 0°C, which is given as 6.02 kJ/mol.
5. Sum the heat required to raise the temperature of ice and the heat of fusion to find the total heat required for the entire process.