(A) Let the rate law be $Rate = k[A]^x[B]^y$.From the data:$1$) $1.2 \times 10^{-3} = k(0.05)^x(0.05)^y$$2$) $2.4 \times 10^{-3} = k(0.10)^x(0.05)^y$$

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(A) Let the rate law be $Rate = k[A]^x[B]^y$.From the data:$1$) $1.2 \times 10^{-3} = k(0.05)^x(0.05)^y$$2$) $2.4 \times 10^{-3} = k(0.10)^x(0.05)^y$$3$) $1.2 \times 10^{-3} = k(0.05)^x(0.10)^y$Dividing equation $(2)$ by $(1)$:$\frac{2.4 \times 10^{-3}}{1.2 \times 10^{-3}} = (\frac{0.10}{0.05})^x$ $\Rightarrow 2 = 2^x$ $\Rightarrow x = 1$.Dividing equation $(3)$ by $(1)$:$\frac{1.2 \times 10^{-3}}{1.2 \times 10^{-3}} = (\frac{0.10}{0.05})^y$ $\Rightarrow 1 = 2^y$ $\Rightarrow y = 0$.Thus,the order with respect to $A$ is $1$ and with respect to $B$ is $0$.

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

Easy

Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$

$0.05$ $0.05$ $1.2 \times 10^{-3}$

$0.10$ $0.05$ $2.4 \times 10^{-3}$

$0.05$ $0.10$ $1.2 \times 10^{-3}$

A
$1$ and $0$
B
$1$ and $1$
C
$0$ and $1$
D
None of these

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

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$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:

$Run$ $[NO]_{0}$ $[Cl_{2}]_{0}$ $r_{0}$

$1$ $0.10$ $0.10$ $0.18$

$2$ $0.10$ $0.20$ $0.35$

$3$ $0.20$ $0.20$ $1.40$

$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).

MediumJEE MAIN 2021

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If the half-life of a reaction is halved when the initial concentration of the reactant is doubled,what is the order of the reaction?

Medium

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For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

Difficult

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Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.

Medium

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$[A] \ (mol/L)$	$[B] \ (mol/L)$	Rate $(mol/L \cdot s)$
$0.05$	$0.05$	$1.2 \times 10^{-3}$
$0.10$	$0.05$	$2.4 \times 10^{-3}$
$0.05$	$0.10$	$1.2 \times 10^{-3}$

$Run$	$[NO]_{0}$	$[Cl_{2}]_{0}$	$r_{0}$
$1$	$0.10$	$0.10$	$0.18$
$2$	$0.10$	$0.20$	$0.35$
$3$	$0.20$	$0.20$	$1.40$

Calculate the order of the reaction with respect to $A$ and $B$ based on the following data: $[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$ $0.05$ $0.05$ $1.2 \times 10^{-3}$ $0.10$ $0.05$ $2.4 \times 10^{-3}$ $0.05$ $0.10$ $1.2 \times 10^{-3}$

Similar Questions

For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

If the half-life of a reaction is halved when the initial concentration of the reactant is doubled,what is the order of the reaction?

For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

Ozone decomposes into oxygen as follows:$O_3 \rightleftharpoons O_2 + [O]$$O_3 + [O] \to 2O_2$ (slow)Determine the order of the reaction $2O_3 \to 3O_2$.

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Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:

$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$

$0.05$ $0.05$ $1.2 \times 10^{-3}$

$0.10$ $0.05$ $2.4 \times 10^{-3}$

$0.05$ $0.10$ $1.2 \times 10^{-3}$

Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.