(A) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[R]_0}{2k}$.Given $[R]_0 = 2 \ M$ and $t_{1/2} = 1 \ h$,we find the rate cons

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(A) For a zero-order reaction,the half-life is given by $t_{1/2} = \frac{[R]_0}{2k}$.Given $[R]_0 = 2 \ M$ and $t_{1/2} = 1 \ h$,we find the rate constant $k = \frac{[R]_0}{2t_{1/2}} = \frac{2}{2 \times 1} = 1 \ M \ h^{-1}$.The time $t$ required for the concentration to change from $[R]_1 = 0.5 \ M$ to $[R]_2 = 0.25 \ M$ is given by $t = \frac{[R]_1 - [R]_2}{k}$.Substituting the values,$t = \frac{0.5 - 0.25}{1} = 0.25 \ h$.

Class 12 Chemistry Chemical Kinetics Zero order reaction

Medium

For a reaction $A \rightarrow$ products,the half-life period is $1 \ h$. The initial concentration of reactant $A$ is $2 \ M$. If this reaction is of zero order,how many hours will it take for the concentration of the reactant to decrease from $0.5 \ M$ to $0.25 \ M$?

A
$0.25$
B
$1$
C
$4$
D
$0.5$

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Chemical Kinetics

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Zero order reaction

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For a reaction $A \rightarrow$ products,the half-life period is $1 \ h$. The initial concentration of reactant $A$ is $2 \ M$. If this reaction is of zero order,how many hours will it take for the concentration of the reactant to decrease from $0.5 \ M$ to $0.25 \ M$?

Similar Questions

The rate constant of the reaction $A \rightarrow B$ is $0.6 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}.$ If the concentration of $A$ is $5 \, M,$ then the concentration of $B$ after $20$ minutes is ......... $M.$

When a graph of concentration $\rightarrow$ Time is plotted for a zero order reaction,the value of the slope is . . . . . . .

The decomposition of $NH_{3}$ on a platinum surface is a zero-order reaction. What are the rates of production of $N_{2}$ and $H_{2}$ if $k = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$?

For a reaction $A \to$ Products,a plot of $\log\,t_{1/2}$ versus $\log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

$2A \xrightarrow{k} B$ is a zero-order reaction, where $k = 1.0 \text{ mol L}^{-1} \text{ min}^{-1}$. If the initial concentration of $A$ is $2 \text{ M}$, then the time taken to complete $75\%$ of the reaction will be (in $\text{ min}$)

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