A coffee cup calorimeter can be used to investigate the process that occurs when solid ammonium nitrate dissolves in water:
NH4NO3 (s) --> NH4+ (aq) + NO3 – (aq)
25.0 g of solid NH4NO3 at 23.0 degrees C is added to 250.0 mL of H2O at the same temperature, and after the solid is all dissolved the temperature is measured to be 15.6 degrees C. Calculate the enthalpy change (in kJ/ mol NH4NO3) for this process. Assume that the density and specific heat capacity of the solution are the same as for water. Is the process endothermic or exothermic?
(I think): q=(c) x (m) x (change in temp)
qsol + qrxn = 0 (or) -qsol = qrxn
The Attempt at a Solution
? I do know that the specific heat for water is 4.184J/g degrees C and its density is 1.000g/mL