(C) The initial rate is given by $R = K[A][B]$.When the concentration of $A$ is kept constant and the concentration of $B$ is doubled,the new concentr

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(C) The initial rate is given by $R = K[A][B]$.When the concentration of $A$ is kept constant and the concentration of $B$ is doubled,the new concentration of $B$ becomes $[B]' = 2[B]$.The new rate $R'$ is given by $R' = K[A][B]' = K[A](2[B])$.Substituting the initial rate expression into the new rate expression,we get $R' = 2 \times (K[A][B]) = 2R$.Therefore,the rate of the reaction is doubled.

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

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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?

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A
It is halved
B
It remains the same
C
It is doubled
D
It is quadrupled

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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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Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

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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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Consider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$
$0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$
$0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$

The value of the rate constant for the above reaction is:

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The half-life period of a $second$ order reaction is:

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Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be

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$[A_2]_0$	$[B_2]_0$	Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$
$0.1 \ M$	$0.1 \ M$	$2.5 \times 10^{-4}$
$0.2 \ M$	$0.1 \ M$	$5.0 \times 10^{-4}$
$0.2 \ M$	$0.2 \ M$	$1.0 \times 10^{-3}$

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?

Similar Questions

Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

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 half-life period of a $second$ order reaction is:

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below: $(i)$ $X_2 \rightarrow X + X$ (fast) $(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow) $(iii)$ $X + Y \rightarrow XY$ (fast) The overall order of the reaction will be

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Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:
$(i)$ $X_2 \rightarrow X + X$ (fast)
$(ii)$ $X + Y_2 \rightleftharpoons XY + Y$ (slow)
$(iii)$ $X + Y \rightarrow XY$ (fast)
The overall order of the reaction will be