(D) Let the order of reaction with respect to $A$ and $B$ be $m$ and $n$ respectively.Then,$rate = k[A]^{m}[B]^{n}$From the table:$2 = k[0.2]^{m}[0.2]

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(D) Let the order of reaction with respect to $A$ and $B$ be $m$ and $n$ respectively.Then,$rate = k[A]^{m}[B]^{n}$From the table:$2 = k[0.2]^{m}[0.2]^{n}$ $(i)$$4 = k[0.2]^{m}[0.4]^{n}$ $(ii)$$36 = k[0.6]^{m}[0.4]^{n}$ $(iii)$On comparing Eqs. $(i)$ and $(ii)$:$\frac{4}{2} = \frac{k[0.2]^{m}[0.4]^{n}}{k[0.2]^{m}[0.2]^{n}}$$2 = (\frac{0.4}{0.2})^{n} = 2^{n}$$n = 1$On comparing Eqs. $(ii)$ and $(iii)$:$\frac{36}{4} = \frac{k[0.6]^{m}[0.4]^{n}}{k[0.2]^{m}[0.4]^{n}}$$9 = (\frac{0.6}{0.2})^{m} = 3^{m}$$3^{2} = 3^{m}$$m = 2$Therefore,the rate law is $r = k[A]^{2}[B]$.

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

Easy

For a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:
Expt. no. $[A]$ $[B]$ Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$ $0.2$ $0.2$ $2$
$2$ $0.2$ $0.4$ $4$
$3$ $0.6$ $0.4$ $36$

Expt. no.	$[A]$	$[B]$	Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$	$0.2$	$0.2$	$2$
$2$	$0.2$	$0.4$	$4$
$3$	$0.6$	$0.4$	$36$

KCET 2012 All KCET

A
$r=k[A][B]^{2}$
B
$r=k[A]^{3}[B]$
C
$r=k[A]^{2}[B]^{2}$
D
$r=k[A]^{2}[B]$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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In the reaction $X \to Y$,if the concentration of reactant $X$ is increased by $1.5$ times,the rate of reaction increases by $1.837$ times. Determine the order of the reaction with respect to $X$.

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If $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)

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The rate law of the reaction $A + 2B \to \text{Product}$ is given by $\frac{d[B]}{dt} = k[B^2]$. If $A$ is taken in excess,the order of the reaction will be

Medium

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For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = K \frac{[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is

Medium

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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 a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:Expt. no.$[A]$$[B]$Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$$1$$0.2$$0.2$$2$$2$$0.2$$0.4$$4$$3$$0.6$$0.4$$36$

Similar Questions

In the reaction $X \to Y$,if the concentration of reactant $X$ is increased by $1.5$ times,the rate of reaction increases by $1.837$ times. Determine the order of the reaction with respect to $X$.

If $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)

The rate law of the reaction $A + 2B \to \text{Product}$ is given by $\frac{d[B]}{dt} = k[B^2]$. If $A$ is taken in excess,the order of the reaction will be

For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = K \frac{[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is

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 a reaction,$A + B \rightarrow$ products,the rate of the reaction at various concentrations is given below. The rate law for the above reaction is:
Expt. no. $[A]$ $[B]$ Rate $(\text{mol} \ \text{dm}^{-3} \ \text{s}^{-1})$
$1$ $0.2$ $0.2$ $2$
$2$ $0.2$ $0.4$ $4$
$3$ $0.6$ $0.4$ $36$