The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction:

AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

When 50.0 mL of 0.100 M AgNO3 is combined with 50.0 mL of 0.100 M HCl in a coffee-cup calorimeter, the temperature changes from 23.40 ∘C∘ to 24.21∘C.

Calculate Enthalpy chnage for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs=4.18J/(g??C) as the specific heat capacity of the solution.

Enthalpy change for the reaction is -67716 J/mol.

Explanation:

Number of moles of in 50.0 mL of 0.100 M of

= Number of moles of HCl in 50.0 mL of 0.100 M of HCl

= moles

= 0.00500 moles

According to balanced equation, 1 mol of reacts with 1 mol of HCl to form 1 mol of AgCl.

So, 0.00500 moles of react with 0.00500 moles of HCl to form 0.00500 moles of AgCl

Total volume of solution = (50.0+50.0) mL = 100.0 mL

So, mass of solution = () g = 100 g

Enthalpy change for the reaction = -(heat released during reaction)/(number of moles of AgCl formed)

=

=

= -67716 J/mol

[m = mass, c = specific heat capacity, = change in temperature and negative sign is included as it is an exothermic reaction]