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In the first order reaction, $75 \%$ of the reactant gets disappeared in 1.386 hours. The rate constant of the reaction is
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Verified Answer
The correct answer is:
$2.8 \times 10^{-4} \mathrm{~s}^{-1}$
For a first order reaction,
$k=\frac{2.303}{1.386 \times 60 \times 60} \log \frac{a}{a-0.75 a}$
$=\frac{2.303}{1.386 \times 60 \times 60} \log 4$
$=2.8 \times 10^{-4} \mathrm{~s}^{-1}$
$k=\frac{2.303}{1.386 \times 60 \times 60} \log \frac{a}{a-0.75 a}$
$=\frac{2.303}{1.386 \times 60 \times 60} \log 4$
$=2.8 \times 10^{-4} \mathrm{~s}^{-1}$
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