In a calorimetry demonstration, 15.0 g of steam at 100 °C is bubbled into a well-insulated container holding an equilibrium mixture consisting of 250 g of ice and 50 g of liquid water, all at 0 °C and 1 atm. Assume that the steam condenses to liquid water at 100 °C and that the resulting liquid water cools to 0 °C without any loss of energy to the surroundings. (Heat capacities are neglected so that all energy exchanges occur through phase changes only.)
For water:
• molar enthalpy of vaporization (100 °C): 40.7 kJ mol⁻¹
• molar enthalpy of fusion (0 °C): 6.01 kJ mol⁻¹
(a) Calculate the quantity of energy released when the steam condenses to liquid water at 100 °C.
(b) Determine the mass of ice that melts as a result of this energy release.
(c) After the system returns to thermal equilibrium at 0 °C, compute the final masses of ice and liquid water present in the container.