(A) Let the rate law be $r = k[A]^x[B]^y$.Comparing experiment $(3)$ and $(1)$:$\frac{0.10}{0.10} = \frac{k[0.024]^x [0.035]^y}{k[0.012]^x [0.035]^y}$

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(A) Let the rate law be $r = k[A]^x[B]^y$.Comparing experiment $(3)$ and $(1)$:$\frac{0.10}{0.10} = \frac{k[0.024]^x [0.035]^y}{k[0.012]^x [0.035]^y}$$1 = (2)^x \implies x = 0$.Comparing experiment $(2)$ and $(3)$:$\frac{0.80}{0.10} = \frac{k[0.024]^x [0.070]^y}{k[0.024]^x [0.035]^y}$$8 = (2)^y \implies y = 3$.Therefore,the rate law is $Rate = k[A]^0[B]^3 = k[B]^3$.

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

Difficult

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

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A
Rate $= k[B]^3$
B
Rate $= k[B]^4$
C
Rate $= k[A][B]^3$
D
Rate $= k[A]^2[B]^2$

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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

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For the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?

MediumMHT CET 2024

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$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

Medium

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The order of a reaction which has the rate expression $\frac{dc}{dt} = K[E]^{3/2}[D]^{3/2}$ is

Medium

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For a reaction: $3X \to 4Y$,calculate the rate of reaction based on the following graph when the concentration of $X$ is $0.1 \ M$.

Difficult

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The reaction $2NO + Br_2 \rightarrow 2NOBr$ follows the mechanism given below:
$(I)$ $NO + Br_2 \rightleftharpoons NOBr_2$ ........ Fast
$(II)$ $NOBr_2 + NO \rightarrow 2NOBr$ ......... Slow
The overall order of this reaction is

Medium

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$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

Similar Questions

For the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$. $Exp. \ No.$ $[A]$ $[B]$ $Rate$ $1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$ $2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$ $3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$ Find out the rate law.

The order of a reaction which has the rate expression $\frac{dc}{dt} = K[E]^{3/2}[D]^{3/2}$ is

For a reaction: $3X \to 4Y$,calculate the rate of reaction based on the following graph when the concentration of $X$ is $0.1 \ M$.

The reaction $2NO + Br_2 \rightarrow 2NOBr$ follows the mechanism given below:$(I)$ $NO + Br_2 \rightleftharpoons NOBr_2$ ........ Fast$(II)$ $NOBr_2 + NO \rightarrow 2NOBr$ ......... SlowThe overall order of this reaction is

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

The reaction $2NO + Br_2 \rightarrow 2NOBr$ follows the mechanism given below:
$(I)$ $NO + Br_2 \rightleftharpoons NOBr_2$ ........ Fast
$(II)$ $NOBr_2 + NO \rightarrow 2NOBr$ ......... Slow
The overall order of this reaction is