In a coffee-cup calorimeter, 50.0ml of 0.100M AgNO3 and50.0ml of 0.100M HCl are mixed to yield the following reaction:

Ag + (aq) + Cl - (ag) >AgCl (s)

The two solutions were initially at 22.60oC, and the final temperature is 23.40oC. Calculate the heat that accompanies this reaction in KJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 g and a specific heat capacity of 4.18 J/oC. g.

-66.88KJ/mol

Explanation:

It is possible to obtain the heat involved in a reaction using a calorimeter. Formula is:

q = - C*m*ΔT

Where q is heat of reaction, C is specific heat capacity (4.18J/°Cg), m is mass of solution (100.0g) and ΔT is temperature change (23.40°C-22.60°C = 0.80°C)

Replacing:

q = - 4.18J/°Cg*100.0g*0.80°C

q = - 334.4J

Now, in the reaction:

Ag⁺ + Cl⁻→ AgCl

AgNO₃ as source of Ag⁺ and HCl as source of Cl⁻

Moles that react are:

0.050L * (0.100mol / L) = 0.0050moles

If 0.0050 moles produce - 334.4J. Heat of reaction is:

-334.4J / 0.0050moles = - 66880J/mol = - 66.88KJ/mol