(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

What is the order of the following reaction: $2 H_2 O_{2(g)} \longrightarrow 2 H_2 O_{(l)} + O_{2(g)}$?

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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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In a one-component second-order reaction,if the concentration of the reactant is reduced to half,the rate

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

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$A$ reaction is first order in $A$ and second order in $B$.
$(i)$ Write the differential rate equation.
$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?
$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?

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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:

Similar Questions

What is the order of the following reaction: $2 H_2 O_{2(g)} \longrightarrow 2 H_2 O_{(l)} + O_{2(g)}$?

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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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,$\frac{d[O_2]}{dt} = K_3[N_2O_5]$What is the relationship between $K_1$,$K_2$,and $K_3$?

$A$ reaction is first order in $A$ and second order in $B$.$(i)$ Write the differential rate equation.$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?

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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:

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

$A$ reaction is first order in $A$ and second order in $B$.
$(i)$ Write the differential rate equation.
$(ii)$ How is the rate affected on increasing the concentration of $B$ three times?
$(iii)$ How is the rate affected when the concentrations of both $A$ and $B$ are doubled?