(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

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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?

TS EAMCET 2022 All TS EAMCET

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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Chemical Kinetics

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First Order reaction

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In a first order reaction,$87.5 \%$ of the reactant is converted into the product in $15 \ minutes$. The rate constant for the reaction is given by:

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If the decomposition reaction $A_{(g)} \longrightarrow B_{(g)}$ follows first-order kinetics,then the graph of the rate of formation of $B$,denoted by $R$,against time $t$ will be:

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If the half-life $(t_{1/2})$ of a reaction is $69.3 \ s$ and the rate constant $(k)$ is $10^{-2} \ s^{-1}$,then the order of the reaction is:

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The half-life of a first-order reaction is $10 \ minutes$. If the initial concentration is $0.08 \ mol/L$ and at some instant the concentration is $0.01 \ mol/L$,then the time elapsed is ...... minutes.

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Initial concentration of reactant in a first order reaction is $0.08 \text{ mol dm}^{-3}$. What concentration would remain after $40 \text{ minutes}$? (Given $\frac{[A]_0}{[A]_t} = 5.00$)

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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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In a first order reaction,$87.5 \%$ of the reactant is converted into the product in $15 \ minutes$. The rate constant for the reaction is given by:

If the decomposition reaction $A_{(g)} \longrightarrow B_{(g)}$ follows first-order kinetics,then the graph of the rate of formation of $B$,denoted by $R$,against time $t$ will be:

If the half-life $(t_{1/2})$ of a reaction is $69.3 \ s$ and the rate constant $(k)$ is $10^{-2} \ s^{-1}$,then the order of the reaction is:

The half-life of a first-order reaction is $10 \ minutes$. If the initial concentration is $0.08 \ mol/L$ and at some instant the concentration is $0.01 \ mol/L$,then the time elapsed is ...... minutes.

Initial concentration of reactant in a first order reaction is $0.08 \text{ mol dm}^{-3}$. What concentration would remain after $40 \text{ minutes}$? (Given $\frac{[A]_0}{[A]_t} = 5.00$)

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