(B) The given rate law is $r = k[A][B]$.Let the initial rate be $r_1 = k[A][B]$.For option $A$: $r_2 = k(2[A])(2[B]) = 4k[A][B] = 4r_1$.For option $B$

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Concentration of $A$ is doubled and concentration of $B$ is kept constant.

(B) The given rate law is $r = k[A][B]$.Let the initial rate be $r_1 = k[A][B]$.For option $A$: $r_2 = k(2[A])(2[B]) = 4k[A][B] = 4r_1$.For option $B$: $r_2 = k(2[A])[B] = 2k[A][B] = 2r_1$.For option $C$: $r_2 = k(0.5[A])(2[B]) = k[A][B] = r_1$.For option $D$: $r_2 = k[A](0.5[B]) = 0.5k[A][B] = 0.5r_1$.Thus,the rate of reaction doubles when the concentration of $A$ is doubled and the concentration of $B$ is kept constant.

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

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Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. The rate of reaction doubles if:

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A
Concentration of both $A$ and $B$ are doubled.
B
Concentration of $A$ is doubled and concentration of $B$ is kept constant.
C
Concentration of $B$ is doubled and concentration of $A$ is halved.
D
Concentration of $A$ is kept constant and concentration of $B$ is halved.

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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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The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)

Easy

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The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$:
$NO_{(g)} + Br_{2(g)} \rightleftharpoons NOBr_{2(g)}$
$NOBr_{2(g)} + NO_{(g)} \longrightarrow 2NOBr_{(g)}$
If the second step is the rate-determining step,the order of the reaction with respect to $NO_{(g)}$ is:

DifficultAIEEE 2006

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For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

Medium

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The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

Medium

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For a certain reaction,the rate constant $K = 2.37 \times 10^2 \ L^2 \ mol^{-2} \ s^{-1}$. What is the order of the reaction?

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Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. The rate of reaction doubles if:

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The order of the reaction occurring by the following mechanism should be:$(i)$ $A_2 \to A + A$ (fast)$(ii)$ $A + B_2 \to AB + B$ (slow)$(iii)$ $A + B \to AB$ (fast)

For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

For a certain reaction,the rate constant $K = 2.37 \times 10^2 \ L^2 \ mol^{-2} \ s^{-1}$. What is the order of the reaction?

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The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)