When $50\mathrm{.}0$ mL of $0\mathrm{.}700$ M of HCl $($aq$)$ is combined with $50\mathrm{.}0$ mL of $0\mathrm{.}600$ M of NaOH $($aq$),$ in a coffee$-$cup calorimeter, the temperature of the solution increases by $4\mathrm{.}00$ Celsius. What is the change in enthalpy for this balanced reaction?

HCl $($aq$)+$ NaOH $($aq$)->$ NaCl $($aq$)+$ H$2$O $($l$)$

Assume that the soluton density is $1\mathrm{.}00$ g$/$mL and the specific heat capacity of the solution is $4\mathrm{.}18$ J$/$gC$.$

A$.47\mathrm{.}8$ kJ

B$.-47\mathrm{.}8$ kJ

C$.55\mathrm{.}8$ kJ

D$.-55\mathrm{.}8$ kJ

E$.-25\mathrm{.}8$ kJ