(A) For a first order reaction,the time $t$ is given by the formula:$t = \frac{2.303}{k} \log \frac{[R]_0}{[R]}$Given $k = 60 \ s^{-1}$ and $[R] = \fr

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(A) For a first order reaction,the time $t$ is given by the formula:$t = \frac{2.303}{k} \log \frac{[R]_0}{[R]}$Given $k = 60 \ s^{-1}$ and $[R] = \frac{[R]_0}{16}$,so $\frac{[R]_0}{[R]} = 16$.Substituting the values:$t = \frac{2.303}{60} \log(16)$$t = \frac{2.303}{60} \times 1.204$$t \approx 0.0462 \ s = 4.62 \times 10^{-2} \ s$.Thus,the required time is $4.62 \times 10^{-2} \ s$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

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

A
$4.6 \times 10^{-2} \ s$
B
$1.0 \times 10^{-2} \ s$
C
$2.3 \times 10^{-2} \ s$
D
$3.2 \times 10^{-2} \ s$

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Chemical Kinetics

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First Order reaction

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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The rate constant of a first order reaction is $15 \times 10^{-3} \ s^{-1}$. How many seconds will $5.0 \ g$ of this reactant take to reduce to $3.0 \ g$?

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At $500\,^oC$,cyclopropane isomerizes to propene. This reaction is first order with a rate constant of $6.7 \times 10^{-4}\,s^{-1}$. If the initial concentration of cyclopropane is $0.05\, M$,what will be the molarity of cyclopropane after $30\, min$ (in $, M$)?

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For a first-order reaction, if the initial concentration $[A]_0 = 1.0 \text{ M}$ and the concentration after time $t = 276 \text{ s}$ is $[A]_t = 0.25 \text{ M}$, find the value of the rate constant $(k)$. (in $\text{ s}^{-1}$)

DifficultMHT CET 2026

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

Similar Questions

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.

The rate constant of a first order reaction is $15 \times 10^{-3} \ s^{-1}$. How many seconds will $5.0 \ g$ of this reactant take to reduce to $3.0 \ g$?

At $500\,^oC$,cyclopropane isomerizes to propene. This reaction is first order with a rate constant of $6.7 \times 10^{-4}\,s^{-1}$. If the initial concentration of cyclopropane is $0.05\, M$,what will be the molarity of cyclopropane after $30\, min$ (in $, M$)?

For a first order reaction,the rate constant is $0.6932 \ hr^{-1}$,then the half-life for the reaction is ......... $hr$.

For a first-order reaction, if the initial concentration $[A]_0 = 1.0 \text{ M}$ and the concentration after time $t = 276 \text{ s}$ is $[A]_t = 0.25 \text{ M}$, find the value of the rate constant $(k)$. (in $\text{ s}^{-1}$)

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