What is the formula to find the value of $t_{1/2}$ for a Zero Order Reaction?

For a certain reaction $R \to \text{Product}$, the plot of concentration $[R]$ vs time has a negative slope as shown. The order of reaction is:

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 $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |

What is the unit for the zero order rate constant?

Mention True $(T)$ and False $(F)$ statement of the following for reaction $R \to P$.
Rate $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$

Which of the following graphs represents a zero order reaction?
($a = $ initial concentration of reactant,
$x = $ concentration of reactant consumed,
$t = $ time)