A calorimeter consists of a massless beaker that contains 20.0 g of solid water (i.e.,
ice) at −30 °C. Then 100.0 g of iron at 70.0 °C are added to the calorimeter. a) Find the
final temperature of the calorimeter after equilibrium is reached. b) If the final
temperature is 0 °C, what fraction of the ice is melted? c) During the process of reaching
thermal equilibrium, how much heat is absorbed by the H2O? by the iron? What is the
sum of these two heats? Why must the sum have this value? [The specific heat of iron is
470 J kg!Cº.]
Anyone good with calorimetry problems?

Question

A calorimeter consists of a massless beaker that contains 20.0 g of solid water (i.e., 
ice) at −30 °C. Then 100.0 g of iron at 70.0 °C are added to the calorimeter. a) Find the 
final temperature of the calorimeter after equilibrium is reached. b) If the final 
temperature is 0 °C, what fraction of the ice is melted? c) During the process of reaching 
thermal equilibrium, how much heat is absorbed by the H2O? by the iron? What is the 
sum of these two heats? Why must the sum have this value? [The specific heat of iron is 
470 J kg!Cº.]
Anyone good with calorimetry problems?