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Chapter 4: Q4.63P (page 180)

8NH3(g)+6NO2(g)鈫�7N2(g)+12H2O(l)Identify the oxidizing agent and the reducing agent in the following reaction, and explain your answer:

Short Answer

Expert verified

Answer: You need to identify the oxidizing agent and reducing agent of the given reaction.

Step by step solution

01

Oxidation state of nitrogen in NH3 

Oxidation state of Hydrogen attached to non-metal is +1.

Let, oxidation state of nitrogen in NH3 is x.

No you can write,

x+3+1=0x=-3

02

Oxidation state of nitrogen in NO2 

Oxidation state of Oxygen attached to non-metal is -2.

Let, oxidation state of nitrogen in NO2 is y.

No you can write,

y+2-2=0y=+4

03

Oxidation state of nitrogen in N2 

Oxidation state of nitrogen in N2 is 0.

04

Conclusion

In the given reaction

8NH3g+6NO2g鈫�7N2g+12H2Ol

The oxidation state of nitrogen in NH3 is -3 which increases to 0 in N2. Therefore, NH3 undergoes oxidation in this given reaction. Hence, it acts as a reducing agent.

The oxidation state of nitrogen in NO2 is +4 which reduces to 0 in N2. Therefore, NO2 undergoes reduction in this given reaction. Hence, it acts as an oxidizing agent.

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