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. $5.0 \times 10^{-2} \mathrm{~s}^{-1}$
  2. $5.0 \times 10^{-3} \mathrm{~s}^{-1}$
  3. $0.5 \times 10^{-2} \mathrm{~s}^{-1}$
  4. $0.5 \times 10^{-3} \mathrm{~s}^{-1}$

Solution

$\mathrm{K}=\frac{0.693}{\mathrm{t}_{1 / 2}}=\frac{0.693}{1386}=0.5 \times 10^{-3} \mathrm{~S}^{-1}$

Asked in: NEET 2009 (Mains)

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