(A) The initial rate is $r_1 = K [A]^2[B]$.When the concentration of $A$ is doubled $([A]_2 = 2[A])$ and the concentration of $B$ is halved $([B]_2 =

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(A) The initial rate is $r_1 = K [A]^2[B]$.When the concentration of $A$ is doubled $([A]_2 = 2[A])$ and the concentration of $B$ is halved $([B]_2 = \frac{[B]}{2})$,the new rate $r_2$ is:$r_2 = K (2[A])^2 \times (\frac{[B]}{2})$$r_2 = K (4[A]^2) \times (\frac{[B]}{2})$$r_2 = 2 \times K [A]^2[B] = 2 \times r_1$Therefore,the reaction rate becomes double.

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

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If a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?

A
Rate becomes double
B
Rate becomes eight times
C
Rate becomes tripled
D
No change in rate

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

Which is the unit of the rate constant for a second-order reaction?

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For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

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If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction becomes $100$ times. What is the order of reaction if the rate law is,$\text{rate} = k[A]^{x}$?

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$

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For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

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If a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?

Similar Questions

Which is the unit of the rate constant for a second-order reaction?

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction becomes $100$ times. What is the order of reaction if the rate law is,$\text{rate} = k[A]^{x}$?

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$

For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.

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