The rate constant for a zero order reaction is $2 \times 10^{-2} \ mol \ L^{-1} \ sec^{-1}$. If the concentration of the reactant after $25 \ sec$ is $0.5 \ M$,the initial concentration must have been ......... $M$.

For a reaction $A \to$ Products,a plot of $\log\,t_{1/2}$ versus $\log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

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?

The reaction $2A \rightarrow B + C$ follows zero-order kinetics when:

For a zero order reaction,the plot of concentration $(a - x)$ $vs$ time is linear with

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