Half life period of a first-order reaction is 1386 seconds. The specific rate constant of the reaction is:

Half life period of a first-order reaction is 1386 seconds. The specific rate constant of the reaction is:
  1. $0.5 \times 10^{-2} \mathrm{~s}^{-1}$
  2. $0.5 \times 10^{-3} \mathrm{~s}^{-1}$
  3. $5.0 \times 10^{-2} \mathrm{~s}^{-1}$
  4. $5.0 \times 10^{-3} \mathrm{~s}^{-1}$

Solution

For a first order reaction
$\mathrm{t}_{1 / 2}=\frac{0.693}{\mathrm{k}} ; \mathrm{k}=\frac{0.693}{1386}=0.5 \times 10^{-3} \mathrm{~s}^{-1}$ ,

Asked in: JEE-TOPICTESTS-CHEMISTRY

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