Question

The value of H° for the reaction below is -72 kJ. ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction.

Answer 1

Answer:

-198 kJ

Explanation:

Hello there!

In this case, as the reaction is not given but we can see that HBr is formed, we can infer that reaction is:

$H_2+Br_2\rightarrow 2HBr$

Whereas the -72 kJ per moles of HBr are:

$\frac{-72kJ}{2molHBr}$

Thus, by multiplying by the formed 5.5 moles of HBr, the total energy release is:

$\frac{-72kJ}{2molHBr} *5.5molHBr\\\\=-198kJ$

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