A student uses a table of average bond energies to calculate the molar enthalpy change for the synthesis of ammonia:

\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightarrow 2\text{NH}_3(\text{g})

The average bond energies are shown in the table below:

Bond	Average bond energy in $kJ/mol\text{kJ/mol}$
$N≡N\text{N}\equiv\text{N}$	945
$H−H\text{H}-\text{H}$	436
$N−H\text{N}-\text{H}$	391

In this reaction:

Each nitrogen molecule ( $N2\text{N}_2$ ) contains one $N≡N\text{N}\equiv\text{N}$ triple bond.
Each hydrogen molecule ( $H2\text{H}_2$ ) contains one $H−H\text{H}-\text{H}$ single bond.
Each ammonia molecule ( $NH3\text{NH}_3$ ) contains three $N−H\text{N}-\text{H}$ single bonds.

Calculate the energy taken in (in $kJ\text{kJ}$ ) when the bonds in the reactants are broken.

Calculate the energy given out (in $kJ\text{kJ}$ ) when the bonds in the products are formed.

Use your answers to (i) and (ii) to calculate the molar enthalpy change, $ΔH\Delta H$ (in $kJ/mol\text{kJ/mol}$ ), for the synthesis of ammonia.