# When N2(g) reacts with H2(g) to form NH3(g) , 92.2 kJ of energy are evolved for each mole of N2(g) that reacts.?

## Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. ++__------+____

Mar 7, 2018

$\frac{1}{2} {N}_{2} \left(g\right) + \frac{3}{2} {H}_{2} \left(g\right) \rightarrow N {H}_{3} \left(g\right) + 46.1 \cdot k J$

#### Explanation:

And according to the terms of the question...

${N}_{2} \left(g\right) + 3 {H}_{2} \left(g\right) \rightarrow 2 N {H}_{3} \left(g\right) + 92.2 \cdot k J$

Enthalpy change is usually quoted per mole of reaction as written. Here it was specified that $92.2 \cdot k J$ is evolved per mole of dinitrogen...

For the lower reaction we could also write $\Delta {H}_{\text{rxn}}^{\circ} = - 92.2 \cdot k J \cdot m o {l}^{-} 1$...