If a 68 gram piece of copper is heated to 100.0oC and then put into a vessel containing 250.0 mL of water at 1.5oC, what will be the final temperature of the water (in oC)?  Take the heat capacity of copper to be 0.385 J/(g oC) and that of H2O(l) to be 4.184 J/(g oC).  Assume the density of water is 1.00 g/mL.

Part A Two substances, A and B, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of substance A is 6.29 g and its initial temperature is 20.7°C.The mass of substance B is 25.9 g and its initial temperature is 52.5 °C. The final temperature of both substances at thermal equilibrium is 46.0°C. If the specific heat capacity of substance B is 1.17 J/(g.°C), what is the specific heat capacity of substance A? Express your answer in joules per gram per degree Celsius. • View Available Hint(s) V ΑΣφ Cs,A J/(g-°C)

The Heat Capacity of Mercury is 0.14 J/g °C. What is the Molar Heat Capacity? J/mol °C

11. A 114.06 mL sample of 0.245 M aqueous hydrochloric acid is added to 122.18 mL of 0.172 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 498.075 J/K. The following reaction occurs when the two solutions are mixed. HCl(aq) + NH3(aq) → NH4Cl(aq) The temperature increase is 2.03°C. Calculate ΔH rxn. Answer=____________________kJ/mol