A $0\mathrm{.}172$ g sample of solid NH$4$ClO$4($s$)$ is dissolved in $152$ mL of water in a coffee cup calorimeter. Once all of the NH$4$ClO$4($s$)$ is dissolved in the water, the final temperature of the solution is found to be $17\mathrm{.}54\backslash$deg C$.$ If the initial temperature of the water in the calorimeter was $24\mathrm{.}14\backslash$deg C$,$ calculate the calorimeter constant $($in J$/$K$)$ for the coffee cup calorimeter.

Report your answer to three significant figures.

The heat of solvation of NH$4$ClO$4($s$)$ is $33\mathrm{.}47$ kJ$/$mol$.$