(A) The rate law is given by $r = k[A_2]^x[B]^y$.From the first two experiments,keeping $[B]$ constant at $0.2 \, M$:$1 \times 10^{-2} = k(0.1)^x(0.2)

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(A) The rate law is given by $r = k[A_2]^x[B]^y$.From the first two experiments,keeping $[B]$ constant at $0.2 \, M$:$1 \times 10^{-2} = k(0.1)^x(0.2)^y$$2 \times 10^{-2} = k(0.2)^x(0.2)^y$Dividing the equations: $2 = (2)^x$,so $x = 1$.From the second and third experiments,keeping $[A_2]$ constant at $0.2 \, M$:$2 \times 10^{-2} = k(0.2)^x(0.2)^y$$8 \times 10^{-2} = k(0.2)^x(0.4)^y$Dividing the equations: $4 = (2)^y$,so $y = 2$.Thus,the order with respect to $A_2$ is $1$ and with respect to $B$ is $2$.

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

Medium

$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

$[A_2]$	$[B]$	$-d[A_2]/dt$
$0.1$	$0.2$	$1 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.2$	$2 \times 10^{-2} \, M \, s^{-1}$
$0.2$	$0.4$	$8 \times 10^{-2} \, M \, s^{-1}$

A
$1, 2$
B
$2, 1$
C
$1, 1$
D
$2, 2$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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$A_2 + 2 \, B \to 2 \, AB$ $[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$ The order of reaction with respect to $A_2$ and $B$ are respectively:

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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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For the reaction,$PCl_5 \longrightarrow PCl_3 + Cl_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively at a given instant. The molar concentration of $PCl_5$ at that instant is

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$A_2 + 2 \, B \to 2 \, AB$

$[A_2]$ $[B]$ $-d[A_2]/dt$

$0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$

$0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$

The order of reaction with respect to $A_2$ and $B$ are respectively:

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?