The rate constant of a first-order reaction i | vedclass

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Question

(A) For a first-order reaction,the rate constant $k$ is given by the formula: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.Given: $k = 1.20 	imes 1

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$426$

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(A) For a first-order reaction,the rate constant $k$ is given by the formula: $k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$.Given: $k = 1.20 	imes 10^{-3} \, s^{-1}$,$[A]_0 = 5 \, g$,and $[A]_t = 3 \, g$.Substituting the values: $1.20 	imes 10^{-3} = \frac{2.303}{t} \log \frac{5}{3}$.$t = \frac{2.303}{1.20 	imes 10^{-3}} 	imes \log(1.666)$.$t = \frac{2.303}{1.20 	imes 10^{-3}} 	imes 0.2218$.$t \approx 425.6 \, s \approx 426 \, s$.

The rate constant of a first-order reaction is $1.20 \times 10^{-3} \, s^{-1}$. How much time will it take for $5 \, g$ of the reactant to reduce to $3 \, g$ (in $, s$)?

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