(B) Let the rate law be $\text{Rate} = K[NH_4^+]^x[NO_2^-]^y$. Comparing experiments $1$ and $2$: $\frac{7.2 \times 10^{-6}}{3.6 \times 10^{-6}} = \le

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(B) Let the rate law be $\text{Rate} = K[NH_4^+]^x[NO_2^-]^y$. Comparing experiments $1$ and $2$: $\frac{7.2 \times 10^{-6}}{3.6 \times 10^{-6}} = \left(\frac{0.24}{0.12}\right)^x \left(\frac{0.10}{0.10}\right)^y$ $2 = (2)^x \implies x = 1$. Comparing experiments $2$ and $3$: $\frac{5.4 \times 10^{-6}}{3.6 \times 10^{-6}} = \left(\frac{0.12}{0.12}\right)^x \left(\frac{0.15}{0.10}\right)^y$ $1.5 = (1.5)^y \implies y = 1$. Thus,the rate law is $\text{Rate} = K[NH_4^+][NO_2^-]$.

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

Medium

For the reaction $NH_4^+ + NO_2^- \to N_2 + 2H_2O$,the experimental data is given below. Determine the rate law for the reaction.
$1.$ $[NH_4^+] = 0.24 \, M, [NO_2^-] = 0.10 \, M, \text{Rate} = 7.2 \times 10^{-6} \, M/s$
$2.$ $[NH_4^+] = 0.12 \, M, [NO_2^-] = 0.10 \, M, \text{Rate} = 3.6 \times 10^{-6} \, M/s$
$3.$ $[NH_4^+] = 0.12 \, M, [NO_2^-] = 0.15 \, M, \text{Rate} = 5.4 \times 10^{-6} \, M/s$

A
$K[NH_4^+]$
B
$K[NH_4^+][NO_2^-]$
C
$K[NH_4^+]^2$
D
$K[NH_4^+][NO_2^-]^{-1}$

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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

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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Identify the order of the following reaction: $2 NO_{2(g)} \longrightarrow 2 NO_{(g)} + O_{2(g)}$

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For a reaction whose rate expression is: Rate $= k[A]^{1/2}[B]^{3/2}$,the order would be

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If the rate law of a reaction $n A \rightarrow B$ is expressed as Rate $= -\frac{1}{n} \frac{d[A]}{dt} = \frac{d[B]}{dt} = k[A]^{x}$,the unit of rate constant $k$ will be:

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For a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would:

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