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A chemical reaction was carried out at 300 K and 280 K . The rate constant were found to be $\mathrm{k}_1$ and $\mathrm{k}_2$ respectively, then
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Verified Answer
The correct answer is:
$k_2=0.25 k_1$
For every $10^{\circ} \mathrm{C}$ rise, rate constant gets doubled. Hence, for every $20^{\circ} \mathrm{C}$ rise, rate constant will be 4 times.
Therefore, according to the given statement,
Temperature $\quad 280 \mathrm{~K} \quad 300 \mathrm{~K}$
Rate constant $\quad \mathrm{k}_2 \quad \mathrm{k}_1\left(4 \mathrm{k}_2\right)$
Thus, $\quad \mathrm{k}_1=4 \mathrm{k}_2 \Rightarrow \mathrm{k}_2=0.25 \mathrm{k}_1$
Therefore, according to the given statement,
Temperature $\quad 280 \mathrm{~K} \quad 300 \mathrm{~K}$
Rate constant $\quad \mathrm{k}_2 \quad \mathrm{k}_1\left(4 \mathrm{k}_2\right)$
Thus, $\quad \mathrm{k}_1=4 \mathrm{k}_2 \Rightarrow \mathrm{k}_2=0.25 \mathrm{k}_1$
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