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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):(d) NO₃⁻(aq) → NO₂⁻(aq)

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shaikhmohd0119

 This is a reduction reaction. The balanced reaction is as follows:

      2e⁻  + 2H⁺ + NO₃⁻ →  NO₂⁻ + H₂O

Rules to balance redox reactions

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

             NO₃⁻(aq) → NO₂⁻(aq)            

Oxidation number of N in NO₃⁻ is 5 while in NO₂⁻, it is 3. Thus there is an decrease in oxidation number, thus reduction is taking place.

  • Now N is balanced on both sides. Balance O by adding H2O

            NO₃⁻ →  NO₂⁻+ H₂O

  • Now balance Hydrogen

          2H⁺ + NO₃⁻ →  NO₂⁻ + H₂O

  • balance charge , +2 and -1 on left and -1 on right. add 2e⁻ on left to balance

        2e⁻  + 2H⁺ + NO₃⁻ →  NO₂⁻ + H₂O

Thus we can conclude that since electrons are lost and reduction takes place.

Learn more about redox reactions at https://brainly.com/question/10203480

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