In lab we did thermochemistry, where we are supposed to find the heats of solution, heat change of calorimeter and molar heat solution of the salt. I calculated that the calorimeter constant for the water we had was 883.194 Joules. We took 1/10 of a mole of NH4Cl and tried to find the calorimetry from there. Our initial temp with 150 mL of deionized water was 23.72 degrees Celsius and after adding 5.349 g of NH4Cl salt, we found the equilibrium temp. to be 21.625 degrees Celsius. How do you calculate Specific Heat of Solution, Heat change of calorimeter, total heat change and molar heat solution of NH4Cl? Any help would be great. Thanks!

Question

In lab we did thermochemistry, where we are supposed to find the heats of solution, heat change of calorimeter and molar heat solution of the salt.  I calculated that the calorimeter constant for the water we had was 883.194 Joules.  We took 1/10 of a mole of NH4Cl and tried to find the calorimetry from there.  Our initial temp with 150 mL of deionized water was 23.72 degrees Celsius and after adding 5.349 g of NH4Cl salt, we found the equilibrium temp. to be 21.625 degrees Celsius. How do you calculate Specific Heat of Solution, Heat change of calorimeter, total heat change and molar heat solution of NH4Cl?  Any help would be great. Thanks!