(D) For a zero-order reaction,the rate law is given by $r = K[A]^0 = K$. Integrating the rate equation,we get $[A]_t = [A]_0 - Kt$. At half-life $(t =

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(D) For a zero-order reaction,the rate law is given by $r = K[A]^0 = K$. Integrating the rate equation,we get $[A]_t = [A]_0 - Kt$. At half-life $(t = t_{1/2})$,the concentration of the reactant $[A]_t = \frac{[A]_0}{2} = \frac{a}{2}$. Substituting these values into the integrated rate equation: $\frac{a}{2} = a - K t_{1/2}$. Rearranging for $t_{1/2}$: $K t_{1/2} = a - \frac{a}{2} = \frac{a}{2}$. Therefore,$t_{1/2} = \frac{a}{2K}$.

Class 12 Chemistry Chemical Kinetics Zero order reaction

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For a reaction,$A \rightarrow B$,the rate equation is $r = K[A]^0$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,find the half-life time of the reaction.

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A
$\frac{a}{4k}$
B
$\frac{a}{k}$
C
$\frac{5a}{2k}$
D
$\frac{a}{2k}$

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For a reaction,$A \rightarrow B$,the rate equation is $r = K[A]^0$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,find the half-life time of the reaction.

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For the zero order reaction $2A \rightarrow B + 3C$,if the rate constant $K = 3.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,what will be the rate of production of $C$?

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Describe the nature of the following graphs for a zero-order reaction:
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time