Rate of a first order reaction is $1.5 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ minute ${ }^{-1}$ at 0…

Rate of a first order reaction is $1.5 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ minute ${ }^{-1}$ at 0.5 M concentration of reactant, calculate half life of reaction.
  1. 0.383 minute
  2. 7.53 minute
  3. 8.73 minute
  4. 23.1 minute

Solution

$\begin{array}{ll} & \text {For a } 1^{\text {st }} \text { order reaction, } \\ & \text { Rate }=\mathrm{k}(\mathrm{A})^1 \\ & 1.5 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \text { minute }^{-1}=\mathrm{k}(0.5 \mathrm{M}) \\ \mathrm{k}=0.03 \text { minute }^{-1}\end{array}$ $\therefore \quad \mathrm{t}_{1 / 2}=\frac{0.693}{0.03 \text { minute }^{-1}}=23.1$ minute

Asked in: MHT CET 2024 (10 May Shift 2)

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