(C) For a first order reaction,the concentration at time $t$ is given by $[A]_t = [A]_0 e^{-kt}$.Given: $[A]_0 = 1 \ M$,$k = 10^{-2} \ sec^{-1}$,$t =

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$5.5 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$

(C) For a first order reaction,the concentration at time $t$ is given by $[A]_t = [A]_0 e^{-kt}$.Given: $[A]_0 = 1 \ M$,$k = 10^{-2} \ sec^{-1}$,$t = 1 \ minute = 60 \ sec$.$[A]_t = 1 \times e^{-(10^{-2} \times 60)} = e^{-0.6}$.Using $e^{-0.6} \approx 0.5488 \ M$.The rate of reaction at time $t$ is $Rate = k[A]_t$.$Rate = 10^{-2} \ sec^{-1} \times 0.5488 \ M = 5.488 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1} \approx 5.5 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

$A$ first order reaction has the rate constant $10^{-2} \ sec^{-1}$. If the initial concentration of reactant is $1 \ M$,then what will be the rate of reaction after $1 \ minute$?

A
$2.6 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$
B
$3.7 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$
C
$5.5 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$
D
$1.9 \times 10^{-3} \ mol \ L^{-1} \ sec^{-1}$

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First Order reaction

$99 \%$ of a first order reaction was completed in $64 \text{ min}$. In how many minutes will $99.9 \%$ of the reaction be complete?

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The rate constant for the decomposition of $H_2O_2$ is $3.66 \times 10^{-3} \ s^{-1}$. If the initial concentration of $H_2O_2$ is $0.882 \ M$,then in how many seconds will its concentration become $0.600 \ M$?

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What is the value of the slope when a graph is plotted of $\log \frac{[R]_0}{[R]}$ versus $t$ (time) for a first-order reaction?

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For the reaction $A \rightarrow B$,the following graph was obtained. The time required (in seconds) for the concentration of $A$ to reduce to $2.5 \ g \ L^{-1}$ (if the initial concentration of $A$ was $50 \ g \ L^{-1}$) is $........$ (Nearest integer). Given: $\log 2 = 0.3010$.

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For the reaction ${N_2}{O_{5(g)}} \to 2N{O_{2(g)}} + \frac{1}{2}{O_{2(g)}}$,the rate constant is $2.3 \times 10^{-2} \ s^{-1}$. Which of the following equations represents the variation of $[{N_2}{O_5}]$ with time?

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$A$ first order reaction has the rate constant $10^{-2} \ sec^{-1}$. If the initial concentration of reactant is $1 \ M$,then what will be the rate of reaction after $1 \ minute$?

Similar Questions

$99 \%$ of a first order reaction was completed in $64 \text{ min}$. In how many minutes will $99.9 \%$ of the reaction be complete?

The rate constant for the decomposition of $H_2O_2$ is $3.66 \times 10^{-3} \ s^{-1}$. If the initial concentration of $H_2O_2$ is $0.882 \ M$,then in how many seconds will its concentration become $0.600 \ M$?

What is the value of the slope when a graph is plotted of $\log \frac{[R]_0}{[R]}$ versus $t$ (time) for a first-order reaction?

For the reaction $A \rightarrow B$,the following graph was obtained. The time required (in seconds) for the concentration of $A$ to reduce to $2.5 \ g \ L^{-1}$ (if the initial concentration of $A$ was $50 \ g \ L^{-1}$) is $........$ (Nearest integer). Given: $\log 2 = 0.3010$.

For the reaction ${N_2}{O_{5(g)}} \to 2N{O_{2(g)}} + \frac{1}{2}{O_{2(g)}}$,the rate constant is $2.3 \times 10^{-2} \ s^{-1}$. Which of the following equations represents the variation of $[{N_2}{O_5}]$ with time?

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