d- and f-Block Elements: Properties, Lanthanoids & Actinoids

(Based on Chemical Kinetics Passage) Calculate the order of a reaction whose $\text{Rate} = k [\text{A}]^{1/2} [\text{B}]^{3/2}$:

(Based on Chemical Kinetics Passage) The rate law of a reaction is given by $r = k[\text{CH}_3\text{OCH}_3]^{3/2}$. If the pressure is measured in bar and time in minutes, then the unit of rate constant will be:

(Based on Chemical Kinetics Passage) If the rate of reaction becomes twenty-seven times upon increasing the concentration of reactant by three times, the order of this reaction is:

For the following reaction: $$2\text{A}_2 (g) + \frac{1}{4} \text{X} (g) \rightarrow 2\text{A}_2\text{X} (g)$$ Volume is increased to double its value by decreasing the pressure on it. If the reaction is first order with respect to $\text{X}$ and second order with respect to $\text{A}_2$, the rate of reaction will:

Identify the order of reaction if its rate constant is $k = 2 \times 10^{-2}\text{ s}^{-1}$:

For a complex reaction, the order of reaction is equal to:

Which of the following is not correct about the order of a reaction?

The rate constant $k$ for a certain reaction is $k = 2.3 \times 10^{-5}\text{ L mol}^{-1}\text{ s}^{-1}$. The order of the reaction is:

The decomposition of $\text{NH}_3$ on platinum surface is a zero order reaction. If $k = 2.5 \times 10^{-4}\text{ mol L}^{-1}\text{ s}^{-1}$, the rate of production of $\text{H}_2$ is:

The molecularity of the following elementary reaction is: $$\text{NH}_4\text{NO}_2 \rightarrow \text{N}_2 + 2\text{H}_2\text{O}$$