(B) Let the rate law be $\text{Rate} = K[A]^x[B]^y$.Using data $1$ and $4$ (where $[B]$ is constant):$\frac{3.0 \times 10^{-2}}{7.5 \times 10^{-3}} =

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(B) Let the rate law be $\text{Rate} = K[A]^x[B]^y$.Using data $1$ and $4$ (where $[B]$ is constant):$\frac{3.0 \times 10^{-2}}{7.5 \times 10^{-3}} = (\frac{0.4}{0.1})^x$ $\Rightarrow 4 = 4^x$ $\Rightarrow x = 1$.Using data $2$ and $3$ (where $[A]$ is constant):$\frac{3.6 \times 10^{-1}}{9.0 \times 10^{-2}} = (\frac{0.4}{0.2})^y$ $\Rightarrow 4 = 2^y$ $\Rightarrow y = 2$.Thus,the rate law is $\text{Rate} = K[A][B]^2$.

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

Easy

For the reaction $2A + B \rightarrow C + D$,select the correct rate law based on the following data:
$1$. $[A] = 0.1, [B] = 0.1, \text{Initial Rate} = 7.5 \times 10^{-3}$
$2$. $[A] = 0.3, [B] = 0.2, \text{Initial Rate} = 9.0 \times 10^{-2}$
$3$. $[A] = 0.3, [B] = 0.4, \text{Initial Rate} = 3.6 \times 10^{-1}$
$4$. $[A] = 0.4, [B] = 0.1, \text{Initial Rate} = 3.0 \times 10^{-2}$

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

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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

For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?

DifficultJEE MAIN 2015

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Identify the reaction intermediate of the following reaction sequence:
$(i)$ $2 SO_{2(g)} + 2 NO_{2(g)} \rightarrow 2 SO_{3(g)} + 2 NO_{(g)}$
$(ii)$ $2 NO_{(g)} + O_{2(g)} \rightarrow 2 NO_{2(g)}$
--------------------------------------------------
Overall: $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$

DifficultMHT CET 2023

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Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?

EasyMHT CET 2025

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In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

Medium

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For a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would:

MediumNEET 2023

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For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?

In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

For a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would:

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