(C) The rate of the reaction is determined by the slow step $(ii)$: $r = k[X][Y_2]$ $---$ $(1)$ From the fast equilibrium step $(i)$,we have: $K_{eq}

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(C) The rate of the reaction is determined by the slow step $(ii)$: $r = k[X][Y_2]$ $---$ $(1)$ From the fast equilibrium step $(i)$,we have: $K_{eq} = \frac{[X]^2}{[X_2]}$ $[X]^2 = K_{eq}[X_2]$ $[X] = K_{eq}^{1/2}[X_2]^{1/2}$ $---$ $(2)$ Substituting equation $(2)$ into equation $(1)$: $r = k \cdot K_{eq}^{1/2}[X_2]^{1/2}[Y_2]^1$ $r = k'[X_2]^{1/2}[Y_2]^1$ The overall order of the reaction is the sum of the exponents of the concentration terms in the rate law: Order $= 0.5 + 1 = 1.5$

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

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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$2$
B
$0$
C
$1.5$
D
$1$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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

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For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

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Fill in the blanks:
$1.$ The rate of reaction depends on the ........... step.
$2.$ In a bimolecular reaction,the reaction takes place with ........... species and ........... .
$3.$ The order of reaction is determined by ...........

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$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

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

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

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

Fill in the blanks:$1.$ The rate of reaction depends on the ........... step.$2.$ In a bimolecular reaction,the reaction takes place with ........... species and ........... .$3.$ The order of reaction is determined by ...........

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

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

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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

Fill in the blanks:
$1.$ The rate of reaction depends on the ........... step.
$2.$ In a bimolecular reaction,the reaction takes place with ........... species and ........... .
$3.$ The order of reaction is determined by ...........