A substance A decomposes by a first order rea | 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: $[A]_0 = 2.00 \, M

Vedclass · Accepted Answer

$1.29 	imes 10^{-2} \, \min^{-1}$

Vedclass · Answer

(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: $[A]_0 = 2.00 \, M$,$[A]_t = 0.15 \, M$,and $t = 200 \, \min$. Substituting the values: $k = \frac{2.303}{200} \log \left( \frac{2.00}{0.15} ight)$ $k = \frac{2.303}{200} \log(13.333)$ $k = \frac{2.303}{200} 	imes 1.1249$ $k \approx 1.29 	imes 10^{-2} \, \min^{-1}$ Therefore,the correct option is $A$.

$A$ substance $A$ decomposes by a first order reaction starting initially with $[A]_0 = 2.00 \, M$ and after $200 \, \min$,$[A]_t = 0.15 \, M$. For this reaction,what is the value of the rate constant $k$?

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