Consider the following reaction:
CaCl2 (s) → Ca2+ (aq) + 2 Cl- (aq) ΔHo = -81.5 kJ
A 38.3 g sample of CaCl2 (MW = 110.98 g/mol) at 0.00 oC is dissolved in a beaker containing 56.5 g of ice (MW = 18.0 g/mol) at 0.00 oC in equilibrium with 101.9 g of water (MW = 18.0 g/mol) at 0.00 oC. Calculate the final temperature of the solution when the CaCl2 has dissolved assuming there is no heat lost to the surroundings, there is no change in the melting point of ice, ΔHfus = 6.02 kJ/mol, and that the solution has a specific heat capacity of 4.184 J/g oC.