Under constant volume conditions, the heat of combustion of benzoic acid, $H{C}_7{H}_5{O}_2,$ is $26\mathrm{.}38k\frac{J}{g}.$ A $1\mathrm{.}200g$ sample of benzoic acid is burned in a bomb calorimeter. What is the total heat change for the reaction?

$=\frac{1\mathrm{.}200(g)}{1}\frac{-26\mathrm{.}38(kJ)}{(g)}$

$q_{\text{c}\text{o}\text{m}\text{b}\text{u}\text{s}\text{t}\text{i}\text{o}\text{n}}=kJ$

Enter either a $+$ or $-$ sign AND the magnitude. Use significant figures.