(B) The rate law for the reaction is given by: $r = k[A]^2 [B]^2$ Substituting the given values: $3.6 \times 10^{-2} = k(0.2)^2 (0.1)^2$ $3.6 \times 1

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$90 \ mol^{-3} \ dm^9 \ sec^{-1}$

(B) The rate law for the reaction is given by: $r = k[A]^2 [B]^2$ Substituting the given values: $3.6 \times 10^{-2} = k(0.2)^2 (0.1)^2$ $3.6 \times 10^{-2} = k(0.04)(0.01)$ $3.6 \times 10^{-2} = k(4 \times 10^{-4})$ $k = \frac{3.6 \times 10^{-2}}{4 \times 10^{-4}} = 0.9 \times 10^2 = 90 \ mol^{-3} \ dm^9 \ sec^{-1}$

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

Medium

For the reaction $A + B \rightarrow$ product,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,find the rate constant of the reaction if it is second order with respect to both reactants.

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A
$18 \ mol^{-3} \ dm^9 \ sec^{-1}$
B
$90 \ mol^{-3} \ dm^9 \ sec^{-1}$
C
$72 \ mol^{-3} \ dm^9 \ sec^{-1}$
D
$36 \ mol^{-3} \ dm^9 \ sec^{-1}$

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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 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?

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State whether the following statements are true $(T)$ or false $(F)$.
$(a)$ In a pseudo first order reaction,the rate and rate constant are determined with respect to the reactant present in lower concentration.
$(b)$ The hydrolysis of an ester is carried out in the presence of an excess of water in an acidic medium.
$(c)$ The hydrolysis of an ester is a second order reaction.

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For the reaction $A + B \rightarrow$ product,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,find the rate constant of the reaction if it is second order with respect to both reactants.

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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?

$2 \ FeCl_3 + SnCl_2 \rightarrow 2 \ FeCl_2 + SnCl_4$. This reaction is an example of:

For a reaction,$K = 4.5 \times 10^{-4} \ L \ mol^{-1} \ s^{-1}$. What is the order of the reaction?

Why is the probability of a reaction with molecularity higher than $3$ very rare?

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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?