Use the following information to answer the next question.

When silver nitrate is made to react with $HCl,$ the hydrogen takes the place of silver in the first compound, as follows:

$AgN{O}_3(aq)+HCl(aq)AgCl(s)+HN{O}_3(aq)$

In a calorimeter, $52\mathrm{.}3mL$ of $0\mathrm{.}642mo\frac{l}{L}AgN{O}_3(aq)$ is mixed with $40\mathrm{.}3mL$ of concentrated $HCl(aq).$

Given that:

the initial temperature of both the solutions $AgN{O}_3$ and $HCl,$ is $18\mathrm{.}9C,$

the highest recorded temperature is $25\mathrm{.}4C,$ after neutralization, and

the density of both the solutions is $1\mathrm{.}00\frac{g}{m}L$

Calculate the enthalpy change for the reaction in $k\frac{J}{m}ol.$