(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

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

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

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

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

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

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

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

AIIMS 2012 All AIIMS

AIIMS 2015 All AIIMS

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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Rate law , Rate constant , Order of Reaction and Molecularity

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The reaction $A_{(g)} + 2B_{(g)} \longrightarrow C_{(g)} + D_{(g)}$ is an elementary process. In an experiment,the initial partial pressure of $A$ and $B$ are $0.6 \ atm$ and $0.8 \ atm$,respectively. When partial pressure of $C$ is $0.2 \ atm$,the rate of reaction relative to the initial rate is

Medium

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Give two examples of zero-order reactions and two examples of first-order reactions.

Medium

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For the reaction $A \to B$,the rate increases by a factor of $2.25$ when the concentration of $A$ is increased by $1.5$. What is the order of the reaction?

Medium

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The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

MediumMHT CET 2023

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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

Medium

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

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The reaction $A_{(g)} + 2B_{(g)} \longrightarrow C_{(g)} + D_{(g)}$ is an elementary process. In an experiment,the initial partial pressure of $A$ and $B$ are $0.6 \ atm$ and $0.8 \ atm$,respectively. When partial pressure of $C$ is $0.2 \ atm$,the rate of reaction relative to the initial rate is

Give two examples of zero-order reactions and two examples of first-order reactions.

For the reaction $A \to B$,the rate increases by a factor of $2.25$ when the concentration of $A$ is increased by $1.5$. What is the order of the reaction?

The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$What is the correct relation between $K$ and $K_1$?

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

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

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

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

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

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

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?