(A) For a first-order reaction,the integrated rate law is given by: $[A]_t = [A]_0 e^{-kt}$ Given that $t = \frac{1}{k}$,we substitute this value into

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(A) For a first-order reaction,the integrated rate law is given by: $[A]_t = [A]_0 e^{-kt}$ Given that $t = \frac{1}{k}$,we substitute this value into the equation: $[A]_t = [A]_0 e^{-k \times (1/k)}$ $[A]_t = [A]_0 e^{-1}$ $[A]_t = \frac{[A]_0}{e}$

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

If the rate law is $r = K[A]$,then the concentration of the reactant remaining after time $t = 1/k$ is: ($[A]_0$ is the concentration of the reactant at $t = 0$)

A
$\frac{[A]_0}{e}$
B
$[A]_0 e$
C
$\frac{[A]_0}{e^2}$
D
$\frac{e}{[A]_0}$

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Chemical Kinetics

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First Order reaction

The rate constant for the oxidation of hydrogen peroxide by $KMnO_4$ is $6.93 \times 10^{-5} \ s^{-1}$. How much time will it take for the volume of a standard $KMnO_4$ solution to decrease from $20 \ mL$ to $8 \ mL$?

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The ratio of the time taken to complete $60\%$ and $20\%$ of a first-order reaction $[A \rightarrow \text{product}]$ is : $(\log 2 = 0.3)$

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The reaction $L \rightarrow M$ starts with $10 \, gL^{-1}$. After $30$ and $90$ minutes,$5 \, gL^{-1}$ and $1.25 \, gL^{-1}$ remain,respectively. The order of the reaction is:

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The reaction $2H_2O_2 \to 2H_2O + O_2$ is a

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Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.
$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$
$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$

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If the rate law is $r = K[A]$,then the concentration of the reactant remaining after time $t = 1/k$ is: ($[A]_0$ is the concentration of the reactant at $t = 0$)

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The rate constant for the oxidation of hydrogen peroxide by $KMnO_4$ is $6.93 \times 10^{-5} \ s^{-1}$. How much time will it take for the volume of a standard $KMnO_4$ solution to decrease from $20 \ mL$ to $8 \ mL$?

The ratio of the time taken to complete $60\%$ and $20\%$ of a first-order reaction $[A \rightarrow \text{product}]$ is : $(\log 2 = 0.3)$

The reaction $L \rightarrow M$ starts with $10 \, gL^{-1}$. After $30$ and $90$ minutes,$5 \, gL^{-1}$ and $1.25 \, gL^{-1}$ remain,respectively. The order of the reaction is:

The reaction $2H_2O_2 \to 2H_2O + O_2$ is a

Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$

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Identify $True$ $(T)$ and $False$ $(F)$ statements of the following for a first order reaction $R \rightarrow P$.
$I. \log \frac{[R]}{[R]_0} = -\frac{kt}{2.303}$
$II. \log \frac{[R]}{[R]_0} = \frac{kt}{2.303}$