(D) The rate law is $R = K[A][B]^2$. At $t = 0$: $[A]_0 = C_0, [B]_0 = 2C_0$. At $t = 30 \min$: $[C] = C_0/4$. From the stoichiometry of the reaction

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(D) The rate law is $R = K[A][B]^2$. At $t = 0$: $[A]_0 = C_0, [B]_0 = 2C_0$. At $t = 30 \min$: $[C] = C_0/4$. From the stoichiometry of the reaction $2A + B \rightarrow C + D$: $[A] = [A]_0 - 2[C] = C_0 - 2(C_0/4) = C_0/2$. $[B] = [B]_0 - [C] = 2C_0 - C_0/4 = 7C_0/4$. Substituting these into the rate law: $R = K(C_0/2)(7C_0/4)^2 = K(C_0/2)(49C_0^2/16) = 49KC_0^3/32$.

Class 12 Chemistry Chemical Kinetics 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:

A
$R = 7C_0^3K/16$
B
$R = 27C_0^3K/32$
C
$R = 247C_0^3K/64$
D
$R = 49KC_0^3/32$

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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

$A$ 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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In the reaction,$P + Q \longrightarrow R + S$,the time taken for $75 \%$ reaction of $P$ is twice the time taken for $50 \%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

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For the elementary reaction $M \rightarrow N$,the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :

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For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

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Which of the following is an elementary reaction?

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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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$A$ 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?

In the reaction,$P + Q \longrightarrow R + S$,the time taken for $75 \%$ reaction of $P$ is twice the time taken for $50 \%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

For the elementary reaction $M \rightarrow N$,the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :

For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

Which of the following is an elementary reaction?

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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?