For a reaction $A \rightarrow P$ at $T \text{ K}$, the half-life $(t_{1/2})$ is plotted as a function of initial concentration $[A]_0$ of $A$ as given below. The value of $x$ in the given figure is . . . . . . $\text{s}$ (Nearest integer).

For a zero order reaction $A \longrightarrow \text{product}$,consider the following graph:
Where $[A_t]$ is the remaining concentration of reactant $A$ at time $t$. Calculate the concentration of $A$ after $2 \ s$. (in $mol/L$)

In the following reaction $A \to B + C,$ the rate constant is $0.001 \ M \ s^{-1}.$ If we start with $1 \ M$ of $A,$ then the concentrations of $A$ and $B$ after $10 \ minutes$ are respectively:

The reaction $2X \to B$ is a zeroth order reaction. If the initial concentration of $X$ is $0.2 \ M$,the half-life is $6 \ h$. When the initial concentration of $X$ is $0.5 \ M$,the time required to reach its final concentration of $0.2 \ M$ will be ........ $hr$.

Mention True $(T)$ and False $(F)$ statements for the following expressions related to a zero-order reaction $R \to P$:
$I. \ k = \frac{[R]_0}{2 t_{1/2}}$
$II. \ t_{1/2} = \frac{[R]_0}{4k}$

$5$ milli-moles of a solid $A$ was dissolved in $5$ moles of $H_2O$. On adding to the solvent,$A$ starts polymerising into another insoluble solid following zero order kinetics. On adding $6$ milli-moles of another solid solute $C$ (after $20$ minutes) the polymerisation completely stops. The insoluble solid polymer is removed and the resulting solution was cooled to a temperature less than $-0.186\,^{\circ}C$ (melting point of solution) to cause solidification of some liquid water. Calculate the value of $'X'$ if rate constant for polymerisation reaction is represented as $10^{-X}\,moles/minute$. $[K_f(H_2O) = 1.86\, K\, Kg\,mol^{-1}]$