(C) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.Rate $= -\frac{d[A]}{dt} = k[A]^0 = k$Integrati

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(C) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.Rate $= -\frac{d[A]}{dt} = k[A]^0 = k$Integrating this expression:$-\int d[A] = \int k dt$$-[A] = kt + C$At $t = 0$,$[A] = [A]_0$,so $C = -[A]_0$.Substituting $C$ back into the equation:$-[A]_t = kt - [A]_0$$[A]_t = [A]_0 - kt$Rearranging for $k$:$kt = [A]_0 - [A]_t$$k = \frac{[A]_0 - [A]_t}{t}$

Class 12 Chemistry Chemical Kinetics Zero order reaction

Medium

Which of the following equations represents the integrated rate law for a zero order reaction?

MHT CET 2021 All MHT CET

A
$k = \frac{[A]_t - [A]_0}{t}$
B
$k = \frac{1}{t} \log_{10} \frac{[A]_0}{[A]_t}$
C
$k = \frac{[A]_0 - [A]_t}{t}$
D
$k = \frac{t}{2.303} \times \log_{10} \frac{[A]_0}{[A]_t}$

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Chemical Kinetics

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Zero order reaction

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Which of the following equations represents the integrated rate law for a zero order reaction?

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Mention True $(T)$ and False $(F)$ statement of the following for reaction $R \to P$.
Rate $= -\frac{d[R]}{dt} = k[R]^0$
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