Question

The rate of the reaction

2 \mathrm{~N}_2 \mathrm{O}_5 \rightarrow 4 \mathrm{NO}_2+\mathrm{O}_2

can be written in three ways:

\begin{aligned} & \frac{-\mathrm{d}\left[\mathrm{N}_2 \mathrm{O}_5\right]}{\mathrm{dt}}={k}\left[\mathrm{~N}_2 \mathrm{O}_5\right] ; \frac{\mathrm{d}\left[\mathrm{NO}_2\right]}{\mathrm{dt}}={k}^{\prime}\left[\mathrm{N}_2 \mathrm{O}_5\right] \\ & \frac{\mathrm{d}\left[\mathrm{O}_2\right]}{\mathrm{dt}}={k}^{\prime \prime}\left[\mathrm{N}_2 \mathrm{O}_5\right] \end{aligned}

The relationship between

{k}

and

{k}^{\prime}

and between

{k}

and

{k}^{\prime \prime}

are:

Accepted Answer

$k^{\prime}=2 k ; k^{\prime \prime}=k / 2$

Answer

$k^{\prime}=2 k ; k^{\prime}=k$

Answer

$k^{\prime}=2 k ; k^{\prime \prime}=2 k$

Answer

$k^{\prime}=k ; k^{\prime \prime}=k$

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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