(D) Let the order of reaction with respect to $A$ and $B$ be $x$ and $y$ respectively.So,the rate law can be given as:$R = k[A]^{x}[B]^{y} \dots (i)$W

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(D) Let the order of reaction with respect to $A$ and $B$ be $x$ and $y$ respectively.So,the rate law can be given as:$R = k[A]^{x}[B]^{y} \dots (i)$When the concentration of only $B$ is doubled,the rate is doubled:$2R = k[A]^{x}[2B]^{y} \dots (ii)$Dividing $(ii)$ by $(i)$:$2 = 2^{y} \Rightarrow y = 1$When concentrations of both $A$ and $B$ are doubled,the rate increases by a factor of $8$:$8R = k[2A]^{x}[2B]^{y} \dots (iii)$Dividing $(iii)$ by $(i)$:$8 = 2^{x} \times 2^{y}$Substituting $y = 1$:$8 = 2^{x} \times 2^{1}$ $\Rightarrow 4 = 2^{x}$ $\Rightarrow x = 2$Thus,the rate law is $R = k[A]^{2}[B]$.

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

In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

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A
rate $= k[A][B]^2$
B
rate $= k[A]^2[B]^2$
C
rate $= k[A][B]$
D
rate $= k[A]^2[B]$

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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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$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

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The rate of a certain reaction is given by,$Rate = k[H^{+}]^n$. The rate increases $100$ times when the $pH$ changes from $3$ to $1$. The order $(n)$ of the reaction is:

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For the reaction $A + B \to C + D$,if the concentration of $A$ is doubled without affecting the concentration of $B$,the rate doubles. If the concentration of $B$ is increased $9$ times without affecting the concentration of $A$,the rate becomes $3$ times. Determine the order of the reaction.

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The rate constant value for a reaction is $1.75 \times 10^2 \ L^2 \ mol^{-2} \ sec^{-1}$. The half-life period $t_{1/2} \propto$ . . . . . . .

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$

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$N_2$ volume in $cc$ $(V_t)$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$ $(V_{\infty})$
Time $(t)$ in minutes	$10$	$15$	$20$	$25$	$\infty$

In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

Similar Questions

$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

The rate of a certain reaction is given by,$Rate = k[H^{+}]^n$. The rate increases $100$ times when the $pH$ changes from $3$ to $1$. The order $(n)$ of the reaction is:

For the reaction $A + B \to C + D$,if the concentration of $A$ is doubled without affecting the concentration of $B$,the rate doubles. If the concentration of $B$ is increased $9$ times without affecting the concentration of $A$,the rate becomes $3$ times. Determine the order of the reaction.

The rate constant value for a reaction is $1.75 \times 10^2 \ L^2 \ mol^{-2} \ sec^{-1}$. The half-life period $t_{1/2} \propto$ . . . . . . .

The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:$N_2$ volume in $cc$ $(V_t)$$6.25$$9.50$$11.42$$13.65$$35.05$ $(V_{\infty})$Time $(t)$ in minutes$10$$15$$20$$25$$\infty$

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$