For the reaction shown, identify the oxidation half-reaction and the reduction half-reaction. KNO3 → KNO2 O2 Which pair of half-reactions represents the balanced half-reactions? First: upper n superscript 5 plus, plus 2 e superscript minus right arrow upper N superscript 3 plus. Second: upper O superscript 2 minus right arrow upper O subscript 2 plus 4 e superscript minus. First: upper n superscript 5 plus plus 4 e superscript minus right arrow 2 upper N superscript 3 plus. Second: 2 upper O superscript 2 minus right arrow upper O subscript 2 plus 4 e superscript minus. First: 4 upper N 5 plus 2 e superscript minus right arrow 4 N superscript 3 plus. Second: 2 upper O superscript 2 minus right arrow 2 Upper O subscript 2 plus 4 e superscript minus.

Explanations:- Oxidation number of nitrogen in nitrate(reactant side) is +5 and in nitrite(product side) it is +3. Here the oxidation number of nitrogen is decreasing from 5 to 3 which is reduction.

As per rules, oxidation number of oxygen in it's compounds is -2 and in elemental form it is 0. So, for the given reaction the oxidation number of oxygen is increasing from -2 to 0 which is oxidation.

The balanced chemical equation is,

Explanation:

cahenny04 cahenny04 · Answer 2 · 2022-03-29T02:15:16+02:00

cahenny04 cahenny04

29-03-2022

Answer:

B

Explanation:

took it on edge

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