Imagine you are performing a calorimetry experiment using a constant-pressure calorimeter. First, you calibrate the calorimeter using the reaction of KOH with HCl (enthalpy = -56.2 kJ/mol). Then, you use the calorimeter to investigate the dissolution of solid ammonium nitrate (NH4NO3). The questions below involve your data (assume the density and specific heat capacity of your solutions is the same as liquid water).
a) A quantity of 85.0mL of 0.600M KOH is mixed with 85.0mL of 0.600M HCl in a coffee-cup calorimeter. The initial temperature of both solutions is 17.36 (degrees celsius), and the final temperature of the mixed solutions is 19.02 (degrees celsius). What is the heat capacity of the calorimeter?
b) A 3.52g sample of NH4NO3 is then dissolved in 80.0mL of water in the same calorimeter, and temperature of the solution changes from 17.54(degrees celcius) to 16.64 (degrees celcius). What is the enthalpy of solution of ammonium nitrate, in kJ/mol?
c) How does the value calculated in part (b) relate to the use of ammonium nitrate in instant cold packs (e.g.,in first aid kits). EXPLAIN BRIEFLY.