रासायनिक बलगतिकी

Read the following passage and answer questions 41 to 45: The speed at which a chemical reaction takes place is called the rate of reaction. The rate of reaction depends on various factors like concentration of the reactants, temperature, etc. The relation between the rate of reaction and the concentration of reacting species is represented by the equation $r = k[\text{A}]^x[\text{B}]^y$, where $x$ and $y$ are the order of the reaction with respect to the reactants A and B, respectively. The overall order of the reaction is $x + y$. The rate of reaction can also be increased by the use of a catalyst which provides an alternate pathway of lower activation energy. It increases the rate of forward and backward reaction to an equal extent. It does not alter the Gibbs energy of the reaction.

The rate of a gaseous reaction is given by $r = k[\text{A}][\text{B}]$. If the volume of the reaction vessel is suddenly reduced to $(1/4)^{\text{th}}$ of its initial value, the reaction rate relating to the initial rate will become:

(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:

(Based on Chemical Kinetics Passage) The role of a catalyst is to change:

If $75\%$ of a first order reaction gets completed in $32\text{ minutes}$, time taken for $50\%$ completion 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:

The half-life of a first order reaction is $25\text{ minutes}$. Its rate constant is:

A drop of solution (volume $0.05\text{ mL}$) contains $3.0 \times 10^{-9}\text{ mole}$ of $\text{H}^+$ ions. If the rate constant of disappearance of $\text{H}^+$ is $1.0 \times 10^{-7}\text{ mol L}^{-1}\text{ s}^{-1}$, how long will it take for $\text{H}^+$ ions to disappear?

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: $$\text{NH}_4\text{NO}_2 \rightarrow \text{N}_2 + 2\text{H}_2\text{O}$$