Statement I :  $\text{A}\to \text{B}\to \text{C}$

For a consecutive chemical reaction shown above the concentration of B increases and then decreases with time.

Statement II : At infinite time, there will be only C in the flask.

The given plots represent the variation of the concentration of a reactant $\mathrm{R}$ with time for two different reactions $\left(\mathrm{i}\right) \mathrm{and} \left(\mathrm{ii}\right)$. The respective orders of the reaction are
(i) 

(ii) 

Two substance $A$($t_{1/2}=5$ mins$)$ and $B$($t_{1/2}=15$ mins) follow first order kinetics are taken in such a way that initially $\left[\mathrm{A}\right]=4[ \mathrm{B}]$. Calculate the time after which the concentration of both the substance will be equal.

Fill your answer as sum of digits till you get the single digit answer.

For each question, enter the correct numerical value (in decimal notation, truncated/rounded off to the second decimal place; e.g. $6.25, 7.00, -0.33, -.30, 30.27, -127.30$, if answer is 11.36777..... then both $11.36777$..... then both $11.36$ and $11.37$ will be correct) by darken the corresponding bubbles in the ORS.

For the elementary reaction $2 \mathrm{A}+{\mathrm{B}}_2⟶2\mathrm{AB}$. Calculate how much the rate of reaction will change if the volume of the vessel is reduced to one third of its original volume?

An exothermic chemical reaction occurs in two steps as follows:

(i) $\mathrm{A}+\mathrm{B}\to \mathrm{X}\mathrm{ }$(fast)

(ii) $\mathrm{ }\mathrm{X}\to \mathrm{AB}\mathrm{ }$(slow)

The progress of the reaction can be best represented by