(A) For a zero order reaction,the rate law is given by: $\text{Rate} = k[A]^0 = k$.Since $\text{Rate} = \frac{d[Concentration]}{dt}$,the unit of the r

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$Concentration \times Time^{-1}$

(A) For a zero order reaction,the rate law is given by: $\text{Rate} = k[A]^0 = k$.Since $\text{Rate} = \frac{d[Concentration]}{dt}$,the unit of the rate constant $(k)$ is the same as the unit of the rate of reaction.Therefore,the unit of the velocity constant is $\frac{\text{Concentration}}{\text{Time}} = \text{Concentration} \times \text{Time}^{-1}$.

Class 12 Chemistry Chemical Kinetics Zero order reaction

Easy

The unit of velocity constant in case of zero order reaction is

A
$Concentration \times Time^{-1}$
B
$Concentration^{-1} \times Time^{-1}$
C
$Concentration \times Time^{2}$
D
$Concentration^{-1} \times Time$

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Class 12

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Chemical Kinetics

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Zero order reaction

If the initial concentration of a reactant is $a$,how much time will it take for a $100\%$ zero-order reaction to complete?

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

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For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained:

$[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$

$t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$

The order of the reaction is:

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If the initial concentration of a reactant is doubled,its half-life period also doubles. Determine the order of the reaction.

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If $c_o$ is the initial concentration of the reactant,what will be the half-life period for a zero-order reaction?

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$[R] \ (M)$	$1.0$	$0.76$	$0.40$	$0.10$
$t \ (min)$	$0.0$	$0.05$	$0.12$	$0.18$

The unit of velocity constant in case of zero order reaction is

Similar Questions

If the initial concentration of a reactant is $a$,how much time will it take for a $100\%$ zero-order reaction to complete?

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

For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained: $[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$ $t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$ The order of the reaction is:

If the initial concentration of a reactant is doubled,its half-life period also doubles. Determine the order of the reaction.

If $c_o$ is the initial concentration of the reactant,what will be the half-life period 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 $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$

For the reaction $R \rightarrow P$,the concentration of $R$ is measured as a function of time and the following data is obtained:

$[R] \ (M)$ $1.0$ $0.76$ $0.40$ $0.10$

$t \ (min)$ $0.0$ $0.05$ $0.12$ $0.18$

The order of the reaction is: