The net enthalpy change of a reaction is the amount of energy required to break all the bonds in reactant molecules minus amount of energy required to form all the bonds in the product molecules. What will be the enthalpy change for the following reaction ? `H_(2) (g) + Br_(2) (g) rarr 2HBr (g)`. Given that, bond energy of `H_(2), Br_(2)` and HBr is `435 kJ mol^(-1), 192 kJ mol^(-1)` and `368 kJ mol^(-1)` respectively

Explanation

To find the enthalpy change (ΔH) for the reaction:

\[ H_2(g) + Br_2(g) \rightarrow 2HBr(g) \]

we will follow these steps:

### Step 1: Identify the bond energies
We are given the bond energies:
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