For the reaction $2 \mathrm{N}_2 \mathrm{O}_5(\mathrm{g}) \rightarrow 4 \mathrm{NO}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}),$ the concentration of $\mathrm{NO}_2$ increases by $2.4 \times 10^{-2} \mathrm{M}$ in $6 \mathrm{~s}.$ What will be the average rate of appearance of $\mathrm{NO}_2$ and the average rate of disappearance of $\mathrm{N}_2 \mathrm{O}_5?$

$2 \times 10^{-3} \mathrm{Ms}^{-1}, 4 \times 10^{-3} \mathrm{Ms}^{-1}$

$2 \times 10^{-3} \mathrm{Ms}^{-1}, 1 \times 10^{-3} \mathrm{Ms}^{-1}$

$2 \times 10 \mathrm{Ms}^{-1}, 2 \times 10^{-3} \mathrm{Ms}^{-1}$

JEE CHEMISTRY MCQ: CHEMICAL KINETICS

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Application +4 | -1

For the reaction

2 \mathrm{N}_2 \mathrm{O}_5(\mathrm{g}) \rightarrow 4 \mathrm{NO}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}),

the concentration of

\mathrm{NO}_2

increases by

2.4 \times 10^{-2} \mathrm{M}

6 \mathrm{~s}.

What will be the average rate of appearance of

\mathrm{NO}_2

and the average rate of disappearance of

\mathrm{N}_2 \mathrm{O}_5?

View answer and explanation

Correct option: D

4 \times 10^{-3} \mathrm{Ms}^{-1}, 2 \times 10^{-3} \mathrm{Ms}^{-1}

Option D (

4 \times 10^{-3} \mathrm{Ms}^{-1}, 2 \times 10^{-3} \mathrm{Ms}^{-1}

) is correct because the average rate of appearance of NO2 and disappearance of N2O5 are calculated based on the stoichiometry of the reaction.