In a coffee cup calorimeter \(50.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{AgNO}_{3}\) and \(50.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{HCl}\) are mixed. The following reaction occurs:

\[\mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{AgCl}(s)\]

If the two solutions are initially at \(22.60^{\circ} \mathrm{C}\), and if the final temperature is \(23.40^{\circ} \mathrm{C}\), calculate \(\Delta H\) for the reaction in \(\mathrm{kJ} / \mathrm{mol}\) of \(\mathrm{AgCl}\) formed. Assume a mass of \(100.0 \mathrm{~g}\) for the combined solution and a specific heat capacity of \(4.18 \mathrm{~J}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}\).