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A chemical reaction was carried out at $300 \mathrm{~K}$ and $280 \mathrm{~K}$. The rate constants were found to be $\mathrm{k}_{1}$ and $\mathrm{k}_{2}$ respectively. Then
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The correct answer is:
$k_{2}^{2}=0.25 \mathrm{k}_{1}$
For every $10^{\circ}$ rise in temperture, Rate gets double. Hence, in this case rate constant will become four time. (d) $i . \mathrm{e}$.,
$$
\begin{array}{l}
k_{1}=4 k_{2} \\
k_{2}=0.25 k_{1}
\end{array}
$$
as the Rise in temperature given is $20^{\circ} \mathrm{C}$
$$
\begin{array}{l}
k_{1}=4 k_{2} \\
k_{2}=0.25 k_{1}
\end{array}
$$
as the Rise in temperature given is $20^{\circ} \mathrm{C}$
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