Which of the following are the correct representations of a zero order reaction,where $[A]$ represents the reactant concentration and $[A]_0$ represents the initial concentration?

For a zero order reaction $A \rightarrow \text{product}$,a plot of $[A]$ (on $y$-axis) and time (on $x$-axis) gave a straight line with slope equal to $-3 \times 10^{-3} \ M \ min^{-1}$ and intercept equal to $2 \times 10^{-2} \ M$ (on $y$-axis). What is the rate constant (in $M \ min^{-1}$) of this reaction?

Which of the following statements is correct about a zero order reaction?

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 $mol/L$)

$A$ zero-order reaction,$A \rightarrow \text{Product}$,with an initial concentration $[A]_0$ has a half-life of $0.2 \ s$. If one starts with the concentration $2[A]_0$,then the half-life is $.... \ s$

The time required for $100 \%$ completion of a zero order reaction is