Problem- Ammonium nitrate is soluble in water. 16.50g of ammonium nitrate is added to an adiabatic calorimeter containing 100.0 g of water initially at 22.0C. The final temperature of the solution is 14.1C.
a) Assuming the heat capacity of the solution is 4.08 J/gC, calculate the molar enthalpy of solvation of ammonium nitrate.
b) Using the table of thermodynamic values at the back of your textbook, calculate the theoretical value of the molar enthalpy of solvation
c) Calculate the percent error for this experimental result.
Anyone can tell me how to solve it step by step so that I will be able to understand what is going on?