(C) The unit of the rate constant $k$ is $s^{-1}$,which indicates that the reaction is a $1^{st}$ order reaction.For a $1^{st}$ order reaction,the int

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Plot of $\ln [A]$ vs $t$ will be a straight line

(C) The unit of the rate constant $k$ is $s^{-1}$,which indicates that the reaction is a $1^{st}$ order reaction.For a $1^{st}$ order reaction,the integrated rate equation is given by $\ln [A] = \ln [A]_0 - kt$.Comparing this with the equation of a straight line $y = mx + c$,where $y = \ln [A]$,$x = t$,$m = -k$ (slope),and $c = \ln [A]_0$ (intercept).Therefore,a plot of $\ln [A]$ versus $t$ will be a straight line with a negative slope equal to $-k$.

Class 12 Chemistry Chemical Kinetics First Order reaction

Medium

The reaction $2A \rightarrow 2B + C$ has a rate constant of $1.2 \times 10^{-2} \ s^{-1}$. Which of the following is correct?

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A
Plot of $[A]$ vs $\frac{1}{t}$ will be a straight line
B
Plot of $\frac{1}{[A]}$ vs $t^2$ will be a straight line
C
Plot of $\ln [A]$ vs $t$ will be a straight line
D
Plot of $[A]$ vs $t^2$ will be a straight line

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Decomposition of $H_2O_2$ follows a first order reaction. In $50 \ min$,the concentration of $H_2O_2$ decreases from $0.5 \ M$ to $0.125 \ M$. For such decomposition,when the concentration of $H_2O_2$ reaches $0.05 \ M$,the rate of formation of $O_2$ will be:

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If $k$ is the rate constant and $t$ is the time,then the degree of dissociation for a substance undergoing decay with first-order kinetics is:

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For a first order reaction,the slope of the graph of $\log_{10}[A]_t$ versus time is equal to:

MediumMHT CET 2020

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What is the half-life time of a first-order reaction if the initial concentration of the reactant is $0.01 \ mol \ L^{-1}$ and the rate of reaction is $0.00352 \ mol \ L^{-1} \ minute^{-1}$?

MediumMHT CET 2023

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If the half-life of a first-order reaction is $6.93$ minutes, then the time required for the completion of $99\%$ of the reaction will be . . . . . . minutes. (Given: $\log 2 = 0.3010$)

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The reaction $2A \rightarrow 2B + C$ has a rate constant of $1.2 \times 10^{-2} \ s^{-1}$. Which of the following is correct?

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Decomposition of $H_2O_2$ follows a first order reaction. In $50 \ min$,the concentration of $H_2O_2$ decreases from $0.5 \ M$ to $0.125 \ M$. For such decomposition,when the concentration of $H_2O_2$ reaches $0.05 \ M$,the rate of formation of $O_2$ will be:

If $k$ is the rate constant and $t$ is the time,then the degree of dissociation for a substance undergoing decay with first-order kinetics is:

For a first order reaction,the slope of the graph of $\log_{10}[A]_t$ versus time is equal to:

What is the half-life time of a first-order reaction if the initial concentration of the reactant is $0.01 \ mol \ L^{-1}$ and the rate of reaction is $0.00352 \ mol \ L^{-1} \ minute^{-1}$?

If the half-life of a first-order reaction is $6.93$ minutes, then the time required for the completion of $99\%$ of the reaction will be . . . . . . minutes. (Given: $\log 2 = 0.3010$)

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