Question #d09f9 Chemistry Electrochemistry Oxidation and Reduction Reactions 1 Answer Nathan L. May 17, 2017 #N# is being oxidized, #H# is being reduced. Explanation: Since #N_2(g)# has an oxidation state of #0# originally, and then has an oxidation state of #+3# on the products side, #N# is being oxidized. Since #H_2(g)# has an oxidation state of #0# originally, and then has an oxidation state of #-1# on the products side, #H# is being reduced. Answer link Related questions How to balance equations for reduction/oxidation reaction? If an electode reaction has dssolved oxygen as a reactant, is the electrode an anode or a cathode? If an electrode reaction has dissolved oxygen as a reactant, is the electrode and anode or a cathode? What balanced equation represents a redox reaction? How are redox reactions involved in electrolysis? Why are oxidation reduction reactions coupled? What do oxidation reduction reactions involve? What are reduction reactions used for? What does "calx" mean in oxidation reduction reactions? What are the reduced components in this reaction? Zn + 2H(+) → Zn(2+) + H2 See all questions in Oxidation and Reduction Reactions Impact of this question 1913 views around the world You can reuse this answer Creative Commons License