(A) For the reaction,$A + B \longrightarrow$ Products.Let the rate law be: $\text{Rate} = k[A]^x[B]^y$.From observation $(i)$,doubling $[A]$ doubles t

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(A) For the reaction,$A + B \longrightarrow$ Products.Let the rate law be: $\text{Rate} = k[A]^x[B]^y$.From observation $(i)$,doubling $[A]$ doubles the rate: $2 \times \text{Rate} = k[2A]^x[B]^y \implies 2 = 2^x \implies x = 1$.From observation $(ii)$,doubling both $[A]$ and $[B]$ increases the rate by a factor of $8$: $8 \times \text{Rate} = k[2A]^1[2B]^y$.Dividing this by the original rate law: $8 = 2^1 \times 2^y \implies 8 = 2 \times 2^y \implies 4 = 2^y \implies y = 2$.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

For the reaction $A + B \rightarrow$ products,it is observed that
$(i)$ on doubling the initial concentration of $A$ only,the rate of reaction is also doubled and
$(ii)$ on doubling the initial concentration of both $A$ and $B$,there is a change by a factor of $8$ in the rate of the reaction.
The rate of this reaction is given by

AIPMT 2009 All AIPMT

A
rate $= k[A][B]^2$
B
rate $= k[A]^2[B]^2$
C
rate $= k[A][B]$
D
rate $= k[A]^2[B]$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.

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The rate of the reaction $x + y \rightarrow \text{product}$ is $5.4 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[x] = 0.2 \ mol \ dm^{-3}$ and $[y] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if it is first order in $X$ and second order in $Y$.

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For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

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The acidic hydrolysis of an ester is a .......

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What is the order of reaction $A + B \to C$?

Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

Observation	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$3.2 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

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For a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.

The rate of the reaction $x + y \rightarrow \text{product}$ is $5.4 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[x] = 0.2 \ mol \ dm^{-3}$ and $[y] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if it is first order in $X$ and second order in $Y$.

For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

The acidic hydrolysis of an ester is a .......

What is the order of reaction $A + B \to C$? Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$

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What is the order of reaction $A + B \to C$?

Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$