Chapter 5.3, Problem 1CP

Given the thermochemical equation: ${\text{ H}}_{\text{2}}\left(g\right){\text{ + Br}}_{\text{2}}\left(l\right)\to \text{2HBr}\left(g\right)\text{, ΔH = –72}\text{.4 kJ/mol}$, calculate the amount

of heat released when a kilogram of ${\text{ Br}}_{\text{2}}\left(l\right)$ is consumed in this reaction.

$\begin{array}{l}\text{a)}\hfill \\ \text{7}\text{.24 }\times {\text{ 10}}^{\text{4}}\text{ kJ}\hfill \\ \text{b)}\hfill \\ \text{453 kJ}\hfill \\ \text{c)}\hfill \\ \text{906 kJ}\hfill \\ \text{d)}\hfill \\ \text{227 kJ}\hfill \\ \text{e)}\hfill \\ \text{724 kJ}\hfill \end{array}$