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The rate of a first order reaction is $1.5 \times 10^{-2} \mathrm{molL}^{-1} \mathrm{~min}^{-1}$ at $0.5 \mathrm{M}$ concentration of the reactant. The half life of the reaction is
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23.1 min
Rate $\left(\frac{d x}{d t}\right)=K \cdot c \quad ; 1.5 \times 10^{-2}=K \times 0.5$
For first order $K=\frac{1.5 \times 10^{-2}}{0.5}=3 \times 10^{-2} \min^{-1}$
$t_{1 / 2}=\frac{.693}{K}=\frac{.693}{3 \times 10^{-2}}=23.1 \mathrm{~min}$
For first order $K=\frac{1.5 \times 10^{-2}}{0.5}=3 \times 10^{-2} \min^{-1}$
$t_{1 / 2}=\frac{.693}{K}=\frac{.693}{3 \times 10^{-2}}=23.1 \mathrm{~min}$
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