Question

The following steps are unbalanced half-reactions involved in the nitrogen cycle. Balance each half-reaction to show the number of electrons lost or gained, and state whether it is an oxidation or a reduction (all occur in acidic conditions):(e) N₂(g) → NO₃⁻(aq)

Answer 1

This is an oxidation reaction. The balanced equation is as follows:

      6H₂O  + N₂ → 2NO₃⁻+ 12H⁺  + 6e⁻

Rules to balance redox reaction in acidic medium

1. Write the given equation in ionic form
2. Identify elements undergoing oxidation ( charge increase, O.N inc) and reduction (charge dec, O.N dec)
3. Break the equation into two halfs
4. Balance the half equations

A. Balance all other atoms except Oxygen and hydrogen

B. Balance oxygen by adding H2O to the side deficient in oxygen

C. Balance hydrogen by adding H+ ions

D. Balance charge by adding electrons

5. Add the two half such that electrons gets cancelled

Oxidation number of N in N2 is 0 while in NO₃⁻, it is +5. Thus there is an increase in oxidation number, thus oxidation is taking place.

              N₂(g) → NO₃⁻(aq)

• balance N.

           N₂ → 2NO₃⁻

• balance O by adding H2O

          6H₂O  + N₂ → 2NO₃⁻

• Now balance Hydrogen

            6H₂O  + N₂ → 2NO₃⁻+ 12H⁺

• balance charge. 0 charge on left, -6 and + 12 on right. add 6e⁻ on right to balance.

             6H₂O  + N₂ → 2NO₃⁻+ 12H⁺  + 6e⁻

Thus we can conclude that since there is increase in oxidation number, oxidation is taking place.

learn more about balancing redox reactions at brainly.com/question/10203480

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