The oxidation of ammonia happens by this reaction: 4NH3(g)+3O2(g)⟶2N2(g)+6H2O(g), if the rate of formation of N2 is 0.5molL−1s−1 then, the rate at which NH3 gets consumed is:
A
1.0molL−1s−1
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B
0.5molL−1s−1
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C
2.0molL−1s−1
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D
1.5molL−1s−1
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Solution
The correct option is A1.0molL−1s−1 The rate of consumption of NH3=−d[NH3]dt
The rate of formation of N2=+d[N2]dt = 0.5molL−1s−1
The rate of the reaction can be written as: −14d[NH3]dt=−13d[O2]dt=12d[N2]dt=16d[H2O]dt −14d[NH3]dt=12d[N2]dt −d[NH3]dt=4×12×0.5=1.0molL−1s−1