Question

Balance the following redox equation, identifying the element oxidized and the element reduced. Show all of the work used to solve the problem.
HNO3 + P ---> H3PO4 + NO

Answer 1

5HNO₃ + 3P + 2H₂O = 3H₃PO₄ + 5NO

N⁺⁵ + 3e⁻ = N⁺²    5
P⁰ - 5e⁻ = P⁺⁵       3

Answer 2

Answer: Phosphorus is getting oxidized and nitrogen is getting reduced.

Explanation:

Oxidation reaction is defined as the reaction in which a substance looses its electron. The oxidation state of the substance gets increased.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

For the given chemical reaction:

$HNO_3+P\rightarrow H_3PO_4+NO$

On reactant side:

Oxidation state of Hydrogen = +1

Oxidation state of Phosphorus = 0

Oxidation state of Nitrogen = +5

Oxidation state of Oxygen = -2

On product side:

Oxidation state of Hydrogen = +1

Oxidation state of Phosphorus = +5

Oxidation state of Nitrogen = +2

Oxidation state of Oxygen = -2

As, the oxidation state of phosphorus is getting increased from 0 to +5, this is getting oxidized and the oxidation state of nitrogen is getting reduced from +5 to +2, this is getting reduced.

Hence, phosphorus is getting oxidized and nitrogen is getting reduced.