(A) The general unit for the rate constant $k$ of an $n^{th}$ order reaction is given by the formula: $(mol \cdot L^{-1})^{1-n} \cdot time^{-1}$.For a

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$time^{-1}, \text{ } mol^{-1} \cdot L \cdot time^{-1}$

(A) The general unit for the rate constant $k$ of an $n^{th}$ order reaction is given by the formula: $(mol \cdot L^{-1})^{1-n} \cdot time^{-1}$.For a first-order reaction $(n=1)$: Unit $= (mol \cdot L^{-1})^{1-1} \cdot time^{-1} = time^{-1}$.For a second-order reaction $(n=2)$: Unit $= (mol \cdot L^{-1})^{1-2} \cdot time^{-1} = (mol \cdot L^{-1})^{-1} \cdot time^{-1} = mol^{-1} \cdot L \cdot time^{-1}$.Thus,the units are $time^{-1}$ and $mol^{-1} \cdot L \cdot time^{-1}$ respectively.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Easy

The rate constants for first-order and second-order reactions have units of ..... respectively.

A
$time^{-1}, \text{ } mol^{-1} \cdot L \cdot time^{-1}$
B
$mol^{-1} \cdot L \cdot time^{-1}, \text{ } time^{-1}$
C
$time^{-1}, \text{ } mol \cdot L^{-1} \cdot time^{-1}$
D
$sec^{-1}, \text{ } L \cdot mol^{-1} \cdot sec^{-1}$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

The experimental data for the reaction $2A + B_2 \to 2AB$ is given below. Determine the rate equation for the reaction.

$Exp.$ $[A]_0$ $[B_2]_0$ $Rate \ (mol \ L^{-1} \ s^{-1})$

$(1)$ $0.50$ $0.50$ $1.6 \times 10^{-4}$

$(2)$ $0.50$ $1.00$ $3.2 \times 10^{-4}$

$(3)$ $1.00$ $1.00$ $3.2 \times 10^{-4}$

MediumAIPMT 1997

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In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

EasyAIPMT 2000

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For a second-order reaction,the rate constant is $8 \times 10^{-5} \, M^{-1} \, \text{min}^{-1}$. In how much time will a $1 \, M$ solution decrease to $0.5 \, M$?

Medium

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For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?

MediumMHT CET 2022

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The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:

Difficult

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$Exp.$	$[A]_0$	$[B_2]_0$	$Rate \ (mol \ L^{-1} \ s^{-1})$
$(1)$	$0.50$	$0.50$	$1.6 \times 10^{-4}$
$(2)$	$0.50$	$1.00$	$3.2 \times 10^{-4}$
$(3)$	$1.00$	$1.00$	$3.2 \times 10^{-4}$

The rate constants for first-order and second-order reactions have units of ..... respectively.

Similar Questions

In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

For a second-order reaction,the rate constant is $8 \times 10^{-5} \, M^{-1} \, \text{min}^{-1}$. In how much time will a $1 \, M$ solution decrease to $0.5 \, M$?

For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?

The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$Then the correct statement is:

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The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is: