Can you help me with this calorimetry problem?

Question

In a coffe cup calorimeter, 50.0mL of 0.100M of AgNO3 and 50mL of 0.100M HCl are mixed to yield the following reaction:

 

Ag+ (aq)  +  Cl -==> AgCl(s)

 

The two solutions were initially at 22.60°C, and the final temperature is 23.40°C. How do I calculate the heat  that accompanies this reaction in kJ/mol, assuming that the combined solution has a mass of 100g and a specific heat capacity of 4.18 J/g°C.

 

 

Answer 1

q = mC∆T

q = heat energy

m = mass = 100 g

C = 4.184 J/g/deg

∆T = change in temperature = 23.4 - 22.60 = 0.8 deg

q = (100 g)(4.184 J/g/deg)(0.8 deg) = 334.72 J

This is the heat for 0.05 L x 0.1 mol/L = 0.005 moles 

To get heat for 1 mole, you have 334.72 J/0.005 moles = 66,944 J/mole = 66.9 kJ/mole