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 $4\mathrm{.}22$ g of CuCl$2($s$)$ are dissolved in $107\mathrm{.}40$ g of water, the temperature of the solution increases from $24\mathrm{.}70$ to $28\mathrm{.}17\backslash$deg C$.$

The heat capacity of the calorimeter $($sometimes referred to as the calorimeter constant$)$ was determined in a separate experiment to be $1\mathrm{.}51$ J$/\backslash$deg C$.$

Based on the student's observation, calculate the enthalpy of dissolution of CuCl$2($s$)$ in kJ$/$mol$.$

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

$\backslash$Delta Hdissolution $=$

kJ$/$mol