When a solid dissolves in water, heat may be evolved or absorbed$.$ The heat of dissolution $($dissolving$)$ can be determined using a coffee cup calorimeter.

In the laboratory a general chemistry student finds that when $7\mathrm{.}63g$ of $N{H}_{4}Br(s)$ are dissolved in $110\mathrm{.}20g$ of water, the temperature of the solution drops from $24\mathrm{.}28$ to $21\mathrm{.}13C.$

The heat capacity of the calorimeter $($sometimes referred to as the calorimeter constant$)$ was determined in a separate experiment to be $1\mathrm{.}73\frac{J}{}C.$

Based on the student's observation, calculate the enthalpy of dissolution of $N{H}_{4}Br(s)$ in $k\frac{J}{m}ol.$

Assume the specific heat of the solution is equal to the specific heat of water.

$H_{\text{d}\text{i}\text{s}\text{s}\text{o}\text{l}\text{u}\text{t}\text{i}\text{o}\text{n}}=,k\frac{J}{m}ol$