(B) For a first order reaction,the rate constant $k$ is given by:$k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$Substituting the given values:$k = \fra

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(B) For a first order reaction,the rate constant $k$ is given by:$k = \frac{2.303}{t} \log \frac{[A]_0}{[A]_t}$Substituting the given values:$k = \frac{2.303}{40} \log \frac{0.1}{0.025}$$k = \frac{2.303}{40} \log 4$$k = \frac{2.303 \times 0.6020}{40} \approx 3.47 \times 10^{-2} \ min^{-1}$The rate of reaction $R$ is given by $R = k[A]$.For $[A] = 0.01 \ M$:$R = (3.47 \times 10^{-2}) \times 0.01$$R = 3.47 \times 10^{-4} \ M/min$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

For a first order reaction $(A) \rightarrow$ products,the concentration of $A$ changes from $0.1 \ M$ to $0.025 \ M$ in $40 \ min$.
The rate of reaction when the concentration of $A$ is $0.01 \ M$ is ............$ \times 10^{-4} \ M/min$.

AIEEE 2012 All AIEEE

A
$0.173$
B
$3.47$
C
$0.347$
D
$1.73$

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For a first order reaction $(A) \rightarrow$ products,the concentration of $A$ changes from $0.1 \ M$ to $0.025 \ M$ in $40 \ min$.The rate of reaction when the concentration of $A$ is $0.01 \ M$ is ............$ \times 10^{-4} \ M/min$.

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$A$ first-order reaction takes $10 \ hours$ to complete $90\%$ of the reaction. How much time will it take to complete $99.9\%$ of the reaction (in $hours$)?

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For a first order reaction $(A) \rightarrow$ products,the concentration of $A$ changes from $0.1 \ M$ to $0.025 \ M$ in $40 \ min$.
The rate of reaction when the concentration of $A$ is $0.01 \ M$ is ............$ \times 10^{-4} \ M/min$.