(A) For a zero-order reaction,the half-life period is given by the formula: $t_{\frac{1}{2}} = \frac{[R]_0}{2k}$.From this expression,it is clear that

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$t_{\frac{1}{2}} \propto [R]_0$

(A) For a zero-order reaction,the half-life period is given by the formula: $t_{\frac{1}{2}} = \frac{[R]_0}{2k}$.From this expression,it is clear that $t_{\frac{1}{2}} \propto [R]_0$,where $[R]_0$ is the initial concentration and $k$ is the rate constant.Therefore,the half-life is directly proportional to the initial concentration of the reactant.

Class 12 Chemistry Chemical Kinetics Zero order reaction

Medium

Which of the following is correct for a zero-order reaction?

A
$t_{\frac{1}{2}} \propto [R]_0$
B
$t_{\frac{1}{2}} \propto \sqrt{[R]_0}$
C
$t_{\frac{1}{2}} \propto [R]_0^2$
D
$t_{\frac{1}{2}} \propto \frac{1}{\sqrt{[R]_0}}$

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Chemical Kinetics

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Zero order reaction

Consider the data given below for the hypothetical reaction $A \to X$:
$Time \ (s)$ $Rate \ (mol \ L^{-1} s^{-1})$
$0$ $1.60 \times 10^{-2}$
$10$ $1.60 \times 10^{-2}$
$20$ $1.60 \times 10^{-2}$
$30$ $1.60 \times 10^{-2}$

From the above data,the order of the reaction is:

$Time \ (s)$	$Rate \ (mol \ L^{-1} s^{-1})$
$0$	$1.60 \times 10^{-2}$
$10$	$1.60 \times 10^{-2}$
$20$	$1.60 \times 10^{-2}$
$30$	$1.60 \times 10^{-2}$

Medium

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For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?
Time $(s)$ Concentration of the reactant $(mol \ L^{-1})$
$0$ $0.1$
$15$ $0.05$
$20$ $0.1 - x$

DifficultAP EAMCET 2022

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What is a zero order reaction? Determine the integrated rate equation for a zero order reaction $R \to P$.

Difficult

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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 ......... $M.$

MediumNEET 2015

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What is the unit of $K$ for a zero-order reaction?

Easy

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Time $(s)$	Concentration of the reactant $(mol \ L^{-1})$
$0$	$0.1$
$15$	$0.05$
$20$	$0.1 - x$

Which of the following is correct for a zero-order reaction?

Similar Questions

Consider the data given below for the hypothetical reaction $A \to X$:$Time \ (s)$$Rate \ (mol \ L^{-1} s^{-1})$$0$$1.60 \times 10^{-2}$$10$$1.60 \times 10^{-2}$$20$$1.60 \times 10^{-2}$$30$$1.60 \times 10^{-2}$From the above data,the order of the reaction is:

For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?Time $(s)$Concentration of the reactant $(mol \ L^{-1})$$0$$0.1$$15$$0.05$$20$$0.1 - x$

What is a zero order reaction? Determine the integrated rate equation for a zero order reaction $R \to P$.

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 ......... $M.$

What is the unit of $K$ for a zero-order reaction?

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Consider the data given below for the hypothetical reaction $A \to X$:
$Time \ (s)$ $Rate \ (mol \ L^{-1} s^{-1})$
$0$ $1.60 \times 10^{-2}$
$10$ $1.60 \times 10^{-2}$
$20$ $1.60 \times 10^{-2}$
$30$ $1.60 \times 10^{-2}$

From the above data,the order of the reaction is:

For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?
Time $(s)$ Concentration of the reactant $(mol \ L^{-1})$
$0$ $0.1$
$15$ $0.05$
$20$ $0.1 - x$