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

1 Answer
anor277
Mar 14, 2016

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

Explanation:

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)#).

Reduction:

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

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)#.

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!

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