A chemical reaction was carried out at $300 \mathrm{~K}$ and $280 \mathrm{~K}$. The rate constants were…
A chemical reaction was carried out at $300 \mathrm{~K}$ and $280 \mathrm{~K}$. The rate constants were found to be $k_{1}$ and $k_{2}$ respectively. then
$k_{2}=4 k_{1}$
$k_{2}=2 k_{1}$
$k_{2}=0.25 k_{1}$
$k_{2}=0.5 k_{1}$
Solution
The rate constant doubles for $10^{\circ} \mathrm{C}$ rise in temperature. For $20^{\circ} \mathrm{C}$ rise, the rate constant will be 4 times $\therefore k_{1}=4 k_{2}$ or $k_{2}=0.25 k_{1}$
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