(D) The rate of the reaction is determined by the slow step,which is the rate-determining step.From step $(ii)$,the rate expression is: Rate $= k_1[M]

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(D) The rate of the reaction is determined by the slow step,which is the rate-determining step.From step $(ii)$,the rate expression is: Rate $= k_1[M][Z]$ ...... $(1)$Since step $(i)$ is a very rapid equilibrium,we can write the equilibrium constant expression:$K_{eq} = \frac{[M]}{[X][Y]}$Therefore,$[M] = K_{eq}[X][Y]$ ...... $(2)$Substituting the value of $[M]$ from equation $(2)$ into equation $(1)$:Rate $= k_1 K_{eq} [X][Y][Z]$Let $k = k_1 K_{eq}$,then the rate law becomes:Rate $= k[X][Y][Z]$

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

Medium

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?

A
Rate $= k[Z]$
B
Rate $= k[X][Y]^2[Z]$
C
Rate $= [N]$
D
Rate $= k[X][Y][Z]$

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Class 12

Chemistry Questions

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

$A$ reaction involving different reactants can never be a/an......?

Easy

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

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

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

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

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

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

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

DifficultAIIMS 2012

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During the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:

$Run$ $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$

$I.$ $0.1$ $0.1$ $6.0 \times 10^{-3}$

$II.$ $0.3$ $0.2$ $7.2 \times 10^{-2}$

$III.$ $0.3$ $0.4$ $2.88 \times 10^{-1}$

$IV.$ $0.4$ $0.1$ $2.40 \times 10^{-2}$

Based on the above data,which one of the following is correct?

AIPMT 2010

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The unit of the rate constant for an $n^{th}$ order reaction is .....

Easy

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The following results have been obtained during the kinetic studies of the reaction:
$2 A + B \rightarrow C + D$

Experiment $[A] / mol \, L^{-1}$ $[B] / mol \, L^{-1}$ Initial rate of formation of $D / mol \, L^{-1} \, min^{-1}$

$I$ $0.1$ $0.1$ $6.0 \times 10^{-3}$

$II$ $0.3$ $0.2$ $7.2 \times 10^{-2}$

$III$ $0.3$ $0.4$ $2.88 \times 10^{-1}$

$IV$ $0.4$ $0.1$ $2.40 \times 10^{-2}$

Determine the rate law and the rate constant for the reaction.

Experiment	$[A] / mol \, L^{-1}$	$[B] / mol \, L^{-1}$	Initial rate of formation of $D / mol \, L^{-1} \, min^{-1}$
$I$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$II$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$III$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$IV$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

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$Run$	$[A] / mol \ L^{-1}$	$[B] / mol \ L^{-1}$	Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$
$I.$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$II.$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$III.$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$IV.$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)$(ii)$ $M + Z \to P$ (slow)$(iii)$ $P + Y \to N$ (very fast)What is the rate law for this reaction?

Similar Questions

$A$ reaction involving different reactants can never be a/an......?

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

The unit of the rate constant for an $n^{th}$ order reaction is .....

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The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?

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

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

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

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

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

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