Q. When 1 mole of ice melts at 0°C and at constant pressure of 1 atm. 1440 calories of heat are absorbed by the system. The molar volumes of ice and water are 0.0196 and 0.0180 litre respectively. Calculate ΔE and ΔH for the reaction.
Attempt:According to the definition, ΔH is the heat supplied at constant pressure, hence in this case ΔH is 1440 calories.
As ΔE=ΔH-PΔV, ΔE is less than 1440 calories but the answer key states that ΔE and ΔH, both are equal to 1440 calories.
Any help is appreciated. Thanks!