Instant hot packs, such as the hand warmers you might use while watching winter sports, might contain solid $CaC{l}_2$ and a pouch of water. When the hot pack is squeezed and folded, the pouch breaks, the $CaC{l}_2$ and water mix, and the solid dissolves, increasing the temperature of the solution by the reaction $CaC{l}_2(s)C{a}^{2+}(aq)+2Cl(aq),$ where the $H_i(CaC{l}_2,(s))=-795\mathrm{.}4k\frac{J}{m}ol,H_i(C{a}^{2+},aq)=-543\mathrm{.}0k\frac{J}{m}ol,$ and $H_i(Cl,aq)=-167\mathrm{.}2k\frac{J}{m}ol.$ If a hot pack contains $103\mathrm{.}5gCaC{l}_2$ and $145\mathrm{.}0g$ of water, what temperature would the hot pack reach if it was activated outside when the temperature is $2\mathrm{.}0C?$ Is this reaction exothermic or endothermic? You can assume the solution has the same specific heat as water $(4\mathrm{.}184\frac{J}{g}*C).$ Also assume there is no heat transfer between the hot pack and the environment.