A 120 g copper calorimeter cup contains 220 cm3 of water and 35 g of ice, all in thermal equilibrium. A 185 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 28 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? (Signs matter!)
C) How much energy is required to raise the temperature of the melted ice and water and copper cup to 28 C? (Signs matter!)
D) How much energy leaves the iron in the form of heat? (Signs Matter!)
E) What was the initial temperature of the iron?