A calorimeter, with calorimeter constant 7.31 J K–1, was used to measure the heat of reaction for mixing 100.0 mL of 0.100 M Ag+ with 100.0 mL of 0.100 M Cl–. The temperature change was +0.770 K for the 200.0 g of solution (specific heat capacity = 4.35 J K–1g–1, density = 1.00 g cm– 3) and the calorimeter.

Question

A calorimeter, with calorimeter constant 7.31 J K–1, was used to measure the heat of reaction for mixing 100.0 mL of 0.100 M Ag+ with 100.0 mL of 0.100 M Cl–. The temperature change was +0.770 K for the 200.0 g of solution (specific heat capacity = 4.35 J K–1g–1, density = 1.00 g cm– 3) and the calorimeter. 
(i) What is the reaction occurring in the calorimeter? (ii) How much heat was absorbed by the calorimeter? (iii)How much heat was absorbed by the solution? (iv) How much heat was released by the reaction? 
(v) What is the heat of reaction per mole of product formed?

DrBob222 · Answer

a. Ag^+(aq) + Cl^-(aq) ==> AgCl(s)
b. q absorbed by calorimeter = Ccal*dT = 7.31 J/K x 0.770 K = ?
c. q absorbed by soln = mcdT = 200 x 4.35 x 0.770 = ?
d. dHrxn = b + c
e. Calculate mols AgCl formed in the reaction and dH in part d will be heat for that many mols AgCl formed. Convert that to dH/1 mol.

Post your work if you get stuck.

S · Answer

Can you please show the working out for e?