(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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Chemical Kinetics

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First Order reaction

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Time required for $90 \%$ completion of a first order reaction is $t$. What is the time required for $99.9 \%$ completion of reaction?

MediumMHT CET 2022

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Following data was obtained for the first order decomposition of $SO_2Cl_{2(g)}$ at constant volume:
$SO_2Cl_{2(g)} \to SO_{2(g)} + Cl_{2(g)}$
$S. No.$ $Time$ $(s)$ $Total$ $pressure$ $(atm)$
$1$ $0$ $0.5$
$2$ $100$ $0.6$

Calculate the rate constant.

Medium

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The ratio of $t_{0.75}$ and $t_{0.5}$ for a first-order reaction is:

Medium

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Derive the half-life $t_{1/2}$ of a first-order reaction.

Difficult

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The rate constant for a first-order reaction is $0.02232 \ min^{-1}$. Calculate the time required for $75 \%$ completion of the reaction. (in $min$)

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$S. No.$	$Time$ $(s)$	$Total$ $pressure$ $(atm)$
$1$	$0$	$0.5$
$2$	$100$	$0.6$

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$.

Similar Questions

Time required for $90 \%$ completion of a first order reaction is $t$. What is the time required for $99.9 \%$ completion of reaction?

Following data was obtained for the first order decomposition of $SO_2Cl_{2(g)}$ at constant volume:$SO_2Cl_{2(g)} \to SO_{2(g)} + Cl_{2(g)}$$S. No.$$Time$ $(s)$$Total$ $pressure$ $(atm)$$1$$0$$0.5$$2$$100$$0.6$Calculate the rate constant.

The ratio of $t_{0.75}$ and $t_{0.5}$ for a first-order reaction is:

Derive the half-life $t_{1/2}$ of a first-order reaction.

The rate constant for a first-order reaction is $0.02232 \ min^{-1}$. Calculate the time required for $75 \%$ completion of the reaction. (in $min$)

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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$.

Following data was obtained for the first order decomposition of $SO_2Cl_{2(g)}$ at constant volume:
$SO_2Cl_{2(g)} \to SO_{2(g)} + Cl_{2(g)}$
$S. No.$ $Time$ $(s)$ $Total$ $pressure$ $(atm)$
$1$ $0$ $0.5$
$2$ $100$ $0.6$

Calculate the rate constant.