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  • Ammonia and oxygen react at higher temperatures as <img alt="4 \mathrm{NH}_3(\mathrm{~g})+5 \mathrm{O}_2(\mathrm{~g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_2 \mathrm{O}(\math

Ammonia and oxygen react at higher temperatures as

4 \mathrm{NH}_3(\mathrm{~g})+5 \mathrm{O}_2(\mathrm{~g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{g})
In an experiment, the concentration of NO increases by 2.16 \times 10^{-2} \mathrm{~mol}$ litre $^{-1} in 3 seconds.
Which of the following is correct?

Option: 1

Rate of the reaction is 7.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}.


Option: 2

Rate of disappearance of ammonia is 7.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}.


Option: 3

Rate of formation of water is 4.32 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}.


Option: 4

Rate of disappearance of oxygen is 3.6 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}.


Answers (1)

best_answer

The rate expression can be written as,
\mathrm{ -\frac{1 d\left[\mathrm{NH}_3\right]}{4 d t}=-\frac{1 d\left[\mathrm{O}_2\right]}{5 d t}=\frac{1 d[N O]}{4 d t}=\frac{1 d\left[\mathrm{H}_2 \mathrm{O}\right]}{6 \mathrm{dt}} }

\mathrm{ r_{\text {reaction }}=\frac{1 d[\mathrm{NO}]}{4 \mathrm{dt}}=\frac{2.16 \times 10^{-2}}{4 \times 3}=1.8 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}

Rate of disappearance of ammonia is \mathrm{=r_{\text {reaction }} \times 4=7.2 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}

Rate of formation of water is \mathrm{=r_{\text {reaction }} \times 6=1.08 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}

Rate of disappearance of oxygen is \mathrm{=r_{\text {reaction }} \times 5=9.0 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}

Posted by

SANGALDEEP SINGH

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