Question

Consider the following redox reaction: 3 NO2 + 3 H2O →2 NO3- + 2 H3O+ +...

Consider the following redox reaction: 3 NO2 + 3 H2O →2 NO3- + 2 H3O+ + NO.

Which species gets oxidized?

Which species gets reduced?

Which species is the oxidizing agent?

Which species is the reducing agent?

Which species gains electrons?

. Which species loses electrons?

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Answer #1

Oxidation number of each element in NO2 is

O=-2

N=+4

Oxidation number of each element in H2O is

H=+1

O=-2

Oxidation number of each element in NO3-1 is

O=-2

N=+5

Oxidation number of each element in NO is

O=-2

N=+2

Oxidation number of each element in H3O+1 is

H=+1

O=-2

So, In short:

Oxidation number of each element in reactant is

O=-2

N=+4

H=+1

Oxidation number of each element in product is

O=-2

N=+2 and +5

H=+1

1)

Nitrogen is getting oxidised

2)

Nitrogen is getting reduced

3)

NO2 is oxidising agent

4)

NO2 is reducing agent

5)

Nitrogen gains electron

6)

Nitrogen loses electron

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