(A) For a first-order reaction,the formula is $t = \frac{2.303}{k} \log \frac{[R]_0}{[R]_t}$.Here,$[R]_0$ is the initial concentration and $[R]_t$ is

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(A) For a first-order reaction,the formula is $t = \frac{2.303}{k} \log \frac{[R]_0}{[R]_t}$.Here,$[R]_0$ is the initial concentration and $[R]_t$ is the concentration at time $t$.Given,$k = 60 \ s^{-1}$ and $[R]_t = \frac{[R]_0}{10}$.Substituting the values: $t = \frac{2.303}{60} \log \frac{[R]_0}{[R]_0/10}$.$t = \frac{2.303}{60} \log(10)$.Since $\log(10) = 1$,$t = \frac{2.303}{60} \approx 3.838 \times 10^{-2} \ s$.

Class 12 Chemistry Chemical Kinetics First Order reaction

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For a first-order reaction,the rate constant is $60 \ s^{-1}$. How much time will it take for the initial concentration of the reactant to be reduced to $1/10$th of its initial value?

A
$3.8 \times 10^{-2} \ s$
B
$1.26 \times 10^{13} \ s$
C
$2.01 \times 10^{13} \ s$
D
$1.097 \times 10^{13} \ s$

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Chemical Kinetics

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First Order reaction

$A$ first order reaction completes $10\%$ of its reaction in $20$ minutes. The time required to complete $19\%$ of the reaction is ........... $\text{min}$.

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The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time (in seconds) will it take to reduce the initial concentration of the reactant to its $1/16^{th}$ value?

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For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?

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The time required for $90\%$ completion of a certain first order reaction is $1 \text{ hour}$. Calculate the time required for $99.9\%$ completion of the same reaction.

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For a first-order reaction $A \to B$,what will be the slope of the graph of $t$ versus $\log(a - x)$?

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For a first-order reaction,the rate constant is $60 \ s^{-1}$. How much time will it take for the initial concentration of the reactant to be reduced to $1/10$th of its initial value?

Similar Questions

$A$ first order reaction completes $10\%$ of its reaction in $20$ minutes. The time required to complete $19\%$ of the reaction is ........... $\text{min}$.

The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time (in seconds) will it take to reduce the initial concentration of the reactant to its $1/16^{th}$ value?

For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?

The time required for $90\%$ completion of a certain first order reaction is $1 \text{ hour}$. Calculate the time required for $99.9\%$ completion of the same reaction.

For a first-order reaction $A \to B$,what will be the slope of the graph of $t$ versus $\log(a - x)$?

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