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

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 $mol/L$)

What is the concentration (in $mol \ L^{-1}$) of the product $B$ after $20 \ s$ in the following reaction? Given that $A \longrightarrow 3B$,rate $= k[A]^0$. The data is provided in the table below:
| Time $(s)$ | Concentration of reactant $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |

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:

For a general reaction $A \to B$,a plot of the concentration of $A$ versus time is given in the figure. Answer the following questions based on this graph:
$(i)$ What is the order of the reaction?
$(ii)$ What is the slope of the curve?
$(iii)$ What are the units of the rate constant?

Which of the following is correct with respect to the graph given?
$\begin{aligned} & [R]=\text{Concentration at time } t \\ & [R]_0=\text{Initial concentration} \end{aligned}$