A 110 g copper calorimeter cup contains 190 cm3 of water and 45 g of ice, all in thermal equilibrium. A 210 g piece of iron is heated to a high temperature and dropped into the water (assume no water escapes the calorimeter cup). At thermal equilibrium the temperature of the entire mixture is 22 C.
A. What is the mass of water before the hot iron is put into the cup?
B. How much energy is required to melt all of the ice?
C. How much energy is required to raise the temperature of the melted ice and water and copper cup to 22 C?