The rate constant of a zero-order reaction is $0.2 \ mol \ L^{-1} \ hr^{-1}$. If the concentration of the reactant after $0.5 \ hr$ is $0.05 \ M$,then the initial concentration of the reactant is ....... $M$.

In a zero-order reaction,if the initial concentration of the reactant is doubled,the time required for half the reactant to be consumed:

Give examples of zero order reactions.

Which of the following is correct with respect to the graph given?
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$

Describe the nature of the following graphs for a zero-order reaction:
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time

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?