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

In the laboratory a general chemistry student finds that when $1\mathrm{.}28g$ of $CaC{l}_2(s)$ are dissolved in $114\mathrm{.}10g$ of water, the temperature of the solution increases from $22\mathrm{.}69$ to $24\mathrm{.}70C.$

The heat capacity of the calorimeter $($sometimes referred to as the calorimeter constant$)$ was determined in a separate experiment to be $1\mathrm{.}58$ J$/\frac{?}{?}C.$

Based on the student's observation, calculate the enthalpy of dissolution of $CaC{l}_2(s)$ in $k\frac{J}{m}ol.$

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

Retry Entire Group

$1$ more group attempt remaining