Zinc metal reacts with hydrochloric acid according to the following balanced equation.

Zn$($s$)+2$HCl$($aq$)->$ZnCl$2($aq$)+$H$2($g$)$

When $0\mathrm{.}111$ g of Zn$($s$)$ is combined with enough HCl to make $53\mathrm{.}2$ mL of solution in a coffee$-$cup calorimeter, all of the zinc reacts, raising the temperature of the solution from $21\mathrm{.}6$C to $24\mathrm{.}7$C$.$ Find $\backslash$Delta rH for this reaction as written. $($Use $1\mathrm{.}0$ gmL$1$ for the density of the solution and $4\mathrm{.}184$ Jg$1$C$1$ as the specific heat capacity.$)$

Express your answer in kilojoules per mole to two significant figures.