Consider the following molecule(X). The major product formed when the given molecule $(X)$ is treated with $\mathrm{HBr}(1\mathrm{eq})$ is :

Given below are two statements : Statement (I) : Alcohols are formed when alkyl chlorides are treated with aqueous potassium hydroxide by elimination reaction. Statement (II) : In alcoholic potassium hydroxide, alkyl chlorides form alkenes by abstracting the hydrogen from the $\beta$-carbon. In the light of the above statements, choose the most appropriate answer from the options given below :

Drug $X$ becomes ineffective after $50 \%$ decomposition. The original concentration of drug in a bottle was $16\mathrm{mg}/\mathrm{mL}$ which becomes $4\mathrm{mg}/\mathrm{mL}$ in 12 months. The expiry time of the drug in months is _________. Assume that the decomposition of the drug follows first order kinetics.

The reaction $A_2+B_2\to 2AB$ follows the mechanism:$A_2\stackrel{k_1}{\underset{k_{-1}}{\rightleftharpoons }}A+A$ (fast)$A+B_2\stackrel{k_2}{\to }AB+B$ (slow)$A+B\to AB$ (fast)The overall order of the reaction is:

Which of the following statement is not true for radioactive decay?

Consider the given figure and choose the correct option :

Consider an elementary reaction $$\mathrm{A}(\mathrm{g})+\mathrm{B}(\mathrm{g})\to \mathrm{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$$ If the volume of reaction mixture is suddenly reduced to $\frac{1}{3}$ of its initial volume, the reaction rate will become ' $x^{\prime }$ times of the original reaction rate. The value of $x$ is :

For bacterial growth in a cell culture, growth law is very similar to the law of radioactive decay. Which of the following graphs is most suitable to represent bacterial colony growth ? Where N - Number of Bacteria at any time, ${\mathrm{N}}_0$ - Initial number of Bacteria.

Which of the following graphs most appropriately represents a zero order reaction?

For a reaction, ${\mathrm{N}}_2{\mathrm{O}}_{5(\mathrm{g})}\to 2{\mathrm{NO}}_{2(\mathrm{g})}+\frac{1}{2}{\mathrm{O}}_{2(\mathrm{g})}$ in a constant volume container, no products were present initially. The final pressure of the system when $50 \%$ of reaction gets completed is

Given below are two statements : Statement (I) : is valid for first order reaction. Statement (II) : is valid for first order reaction. In the light of the above statements, choose the correct answer from the options given below :

For a given reaction $\mathrm{R}\to \mathrm{P},{\mathrm{t}}_{1/2}$ is related to $[\mathrm{A}{]}_0$ as given in table. Given: $\log 2=0.30$ Which of the following is true? A. The order of the reaction is $1 / 2$. B. If $[\mathrm{A}{]}_0$ is 1 M , then ${\mathrm{t}}_{1/2}$ is $200\sqrt{10}\min$ C. The order of the reaction changes to 1 if the concentration of reactant changes from 0.100 M to 0.500 M. D. ${\mathrm{t}}_{1/2}$ is 800 min for $[\mathrm{A}{]}_0=1.6\mathrm{M}$ Choose the correct answer from the options given below:

In a first order decomposition reaction, the time taken for the decomposition of reactant to one fourth and one eighth of its initial concentration are $t_1$ and $t_2$ (s), respectively. The ratio $t_1/t_2$ will be:

A person's wound was exposed to some bacteria and then bacterial growth started to happen at the same place. The wound was later treated with some antibacterial medicine and the rate of bacterial decay(r) was found to be proportional with the square of the existing number of bacteria at any instance. Which of the following set of graphs correctly represents the 'before' and 'after' situation of the application of the medicine? [Given: $N=$ No. of bacteria, $t=$ time, bacterial growth follows $1^{\text{st }}$ order kinetics.]

Reaction $\mathrm{A}(\mathrm{g})\to 2\mathrm{B}(\mathrm{g})+\mathrm{C}(\mathrm{g})$ is a first order reaction. It was started with pure A .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-7btt{border-color:inherit;font-weight:bold;text-align:center;vertical-align:top} .tg .tg-0pky{border-color:inherit;text-align:left;vertical-align:top} t/min Pressure of system at time t/mm Hg 10 160 $\infty$ 240 Which of the following option is incorrect?

Reactant A converts to product D through the given mechanism (with the net evolution of heat): A → B slow; ΔH = +ve B → C fast; ΔH = -ve C → D fast; ΔH = -ve Which of the following represents the above reaction mechanism?

In a reaction $A+B\to C$, initial concentrations of $A$ and $B$ are related as $[A{]}_0=8[B{]}_0$. The half lives of $A$ and $B$ are 10 min and 40 min , respectively. If they start to disappear at the same time, both following first order kinetics, after how much time will the concentration of both the reactants be same?

Consider the following plots of $\log$ of rate constant $\mathrm{k}(\log \mathrm{k})$ vs $\frac{1}{\mathrm{T}}$ for three different reactions. The correct order of activation energies of these reactions is :

Half life of zero order reaction $\mathrm{A}\to$ product is 1 hour, when initial concentration of reactant is $2.0\mathrm{mol}\mathrm{L}{}^{-1}$. The time required to decrease concentration of A from 0.50 to $0.25\mathrm{mol}{\mathrm{L}}^{-1}$ is :