# Can you represent the reduction of dinitrogen pentoxide by dihydrogen gas?

Mar 14, 2016

${N}_{2} {O}_{5} \left(g\right) + 8 {H}_{2} \left(g\right) \rightarrow 2 N {H}_{3} \left(g\right) + 5 {H}_{2} O \left(l\right)$

#### Explanation:

This a redox equation in which nitrogen ($N \left(V\right)$) is reduced to ammonia ($N \left(I I I\right)$), and zerovalent hydrogen gas ($H \left(0\right)$) is oxidized to water and ammonia ($H \left(I\right)$).

Reduction:

${N}_{2} {O}_{5} \left(g\right) + 16 {H}^{+} + 16 {e}^{-} \rightarrow 2 N {H}_{3} \left(g\right) + 5 {H}_{2} O \left(l\right)$ $\left(i\right)$

Oxidation:

${H}_{2} \left(g\right) \rightarrow 2 {H}^{+} + 2 {e}^{-}$ $\left(i i\right)$

$\left(i\right) + 8 \times \left(i i\right)$

${N}_{2} {O}_{5} \left(g\right) + 8 {H}_{2} \left(g\right) \rightarrow 2 N {H}_{3} \left(g\right) + 5 {H}_{2} O \left(l\right)$.

I must admit that I balanced this directly. However, formal consideration of the redox couple does give the required stoichiometry. As for any equation, both mass and charge are BALANCED. This a rather expensive way to make ammonia!