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

Question

Wyatt Atkins · Accepted Answer

#N_2O_5(g) + 8H_2(g) rarr 2NH_3(g) + 5H_2O(l)#

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

Decrease:

#N_2O_5(g) + 16H^+ + 16e^(-) rarr 2NH_3(g) + 5H_2O(l)# #(i)#

The process of oxidation

#H_2(g) rarr 2H^+ + 2e^-# #(ii)#

#(i) + 8xx(ii)#

#N_2O_5(g) + 8H_2(g) rarr 2NH_3(g) + 5H_2O(l)#.

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

Serenity Allen · Answer

undefined Sure, the reduction of dinitrogen pentoxide ($N_2O_5$) by dihydrogen gas ($H_2$) can be represented by the following equation:

$$ N_2O_5 + 2H_2 \rightarrow 2HNO_3 $$

This reaction forms two molecules of nitric acid ($HNO_3$).