Ncert Exercises & Solutions

In the preparation of ${HNO}_{3}$ , we get $NO$ gas by catalytic oxidation of ammonia. The moles of NO produced by the oxidation of two moles of ${NH}_{3}$ will be:

1.	2	2.	3
3.	4	4.	6

Hint: $\mathrm{NH}_{3} + \mathrm{O}_{2} \xrightarrow[Pt/Rh \ gauge \ catalyst]{\Delta } \mathrm{NO}(\mathrm{g})+ \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$

When oxidation of NH₃ takes place then NO is obtained as a product. The balanced equation is as follows:

$4 \mathrm{NH}_{3}+5 \mathrm{O}_{2} \xrightarrow[Pt/Rh \ gauge \ catalyst]{\Delta } 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$
From the reaction, it is clear that 4 moles of NH₃ produce 4 moles of NO. Thus, 2 moles of NH₃ produces 2 moles of NO.

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