(B) The general rate law is given by: $\text{Rate} = K[A]^x[B]^y$. When the concentration of $A$ is doubled,the rate increases by $4$ times $(2^2 = 4)

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(B) The general rate law is given by: $\text{Rate} = K[A]^x[B]^y$. When the concentration of $A$ is doubled,the rate increases by $4$ times $(2^2 = 4)$,which implies the order with respect to $A$ is $x = 2$. When the concentration of $B$ is doubled,the rate remains unchanged,which implies the order with respect to $B$ is $y = 0$. Substituting these values into the rate law: $\text{Rate} = K[A]^2[B]^0 = K[A]^2$.

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

Medium

For the reaction $A + B \rightarrow$ products,doubling the concentration of $A$ increases the reaction rate by four times,but doubling the concentration of $B$ has no effect on the reaction rate. What is the rate law?

A
Rate $= K[A][B]$
B
Rate $= K[A]^2$
C
Rate $= K[A]^2[B]$
D
Rate $= K[A]^2[B]^2$

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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

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

Medium

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Calculate the overall order of a reaction which has the rate expression:
$(a)$ $\text{Rate} = k[A]^{1/2}[B]^{3/2}$
$(b)$ $\text{Rate} = k[A]^{3/2}[B]^{-1}$

Medium

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In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

Medium

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For an $n^{th}$ order reaction,the rate law is given by $\frac{dx}{dt} = K[A]^n$. Which parameter can be determined from the logarithmic plot?

Medium

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The experimental data for the reaction $2A + B_2 \to 2AB$ is given below. Determine the rate equation for the reaction.

$Exp.$ $[A]_0$ $[B_2]_0$ $Rate \ (mol \ L^{-1} \ s^{-1})$

$(1)$ $0.50$ $0.50$ $1.6 \times 10^{-4}$

$(2)$ $0.50$ $1.00$ $3.2 \times 10^{-4}$

$(3)$ $1.00$ $1.00$ $3.2 \times 10^{-4}$

MediumAIPMT 1997

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$Exp.$	$[A]_0$	$[B_2]_0$	$Rate \ (mol \ L^{-1} \ s^{-1})$
$(1)$	$0.50$	$0.50$	$1.6 \times 10^{-4}$
$(2)$	$0.50$	$1.00$	$3.2 \times 10^{-4}$
$(3)$	$1.00$	$1.00$	$3.2 \times 10^{-4}$

For the reaction $A + B \rightarrow$ products,doubling the concentration of $A$ increases the reaction rate by four times,but doubling the concentration of $B$ has no effect on the reaction rate. What is the rate law?

Similar Questions

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

Calculate the overall order of a reaction which has the rate expression:$(a)$ $\text{Rate} = k[A]^{1/2}[B]^{3/2}$$(b)$ $\text{Rate} = k[A]^{3/2}[B]^{-1}$

In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

For an $n^{th}$ order reaction,the rate law is given by $\frac{dx}{dt} = K[A]^n$. Which parameter can be determined from the logarithmic plot?

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Calculate the overall order of a reaction which has the rate expression:
$(a)$ $\text{Rate} = k[A]^{1/2}[B]^{3/2}$
$(b)$ $\text{Rate} = k[A]^{3/2}[B]^{-1}$