(D) The rate law for the reaction $A \to B$ is given by $r = k[A]^x$,where $x$ is the order of reaction.For the first condition: $2.40 \times 10^{-4}

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(D) The rate law for the reaction $A \to B$ is given by $r = k[A]^x$,where $x$ is the order of reaction.For the first condition: $2.40 \times 10^{-4} = k(2 \times 10^{-3})^x$ $(i)$For the second condition: $0.60 \times 10^{-4} = k(1 \times 10^{-3})^x$ $(ii)$Dividing equation $(i)$ by equation $(ii)$:$\frac{2.40 \times 10^{-4}}{0.60 \times 10^{-4}} = \frac{k(2 \times 10^{-3})^x}{k(1 \times 10^{-3})^x}$$4 = (2)^x$Since $4 = 2^2$,we have $x = 2$.Therefore,the order of reaction with respect to $A$ is $2$.

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

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In a chemical reaction $A$ is converted into $B$. The rates of reaction,starting with initial concentrations of $A$ as $2 \times 10^{-3} \ M$ and $1 \times 10^{-3} \ M$,are equal to $2.40 \times 10^{-4} \ M s^{-1}$ and $0.60 \times 10^{-4} \ M s^{-1}$ respectively. The order of reaction with respect to reactant $A$ will be

AIEEE 2012 All AIEEE

A
$0$
B
$1.5$
C
$1$
D
$2$

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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

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State whether the following sentences are true $(T)$ or false $(F)$:
$(a)$ There is more than one reactant in a pseudo first order reaction.
$(b)$ In a pseudo first order reaction,the concentration of both reactants is the same.
$(c)$ In a pseudo first order reaction,the concentration of one reactant is very high.

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What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$

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If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

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For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

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The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

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What is the molecularity of the following reactions?$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$

If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

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What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$