I took out an ice cube from the -10°C freezer and wanted to add it to the drink, but was immediately called away and forgot to add it to the drink. When I came back, I saw that the ice cube had completely melted into water at a room temperature of 25°C. Assuming that the ice cube is exactly 2 mole, and regard this ice cube as a system, try to calculate the change of enthalpy and entropy (△H,△S) of the system. Let the heat capacity of water be 25 JK-1mol-1, the heat capacity of ice be 15 JK-1mol-1 and the heat of melting of ice △Ĥfus = 6 kJ/mol.

I took out an ice cube from the -10°C freezer and wanted to add it to the drink, but was immediately called away and forgot to add it to the drink. When I came back, I saw that the ice cube had completely melted into water at a room temperature of 25°C. Assuming that the ice cube is exactly 2 mole, and regard this ice cube as a system, try to calculate the change of enthalpy and entropy (△H,△S) of the system. Let the heat capacity of water be 25 JK^-1mol^-1, the heat capacity of ice be 15 JK^-1mol^-1 and the heat of melting of ice △Ĥ_fus = 6 kJ/mol.