In a coffee$-$cup calorimeter, $120\mathrm{.}0$ mL of $1\mathrm{.}2$ M and $120\mathrm{.}0$ mL of $1\mathrm{.}2$ M are mixed. Both solutions were originally at $26\mathrm{.}3\backslash$deg C$.$ After the reaction, the final temperature is $34\mathrm{.}3\backslash$deg C$.$ Assuming that all the solutions have a density of $1\mathrm{.}0$ and a specific heat capacity of $4\mathrm{.}18$ J$/\backslash$deg C$$g$,$ calculate the enthalpy change for the neutralization of by $.$ Assume that no heat is lost to the surroundings or to the calorimeter.

$\backslash$Delta H $=$ kJ$/$mol