When a graph of concentration $\rightarrow$ Time is plotted for a zero order reaction,the value of the slope is . . . . . . .

The rate constant for a zero order reaction is $3 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. After $25 \ s$,if the concentration of the reactant is $0.5 \ M$,then the initial concentration of the reactant is ............ $M$.

Which of the following is the incorrect equation for the rate constant of a zero-order reaction?

The rate constant of a zero-order reaction is $0.2 \ mol \ m^{-3} \ h^{-1}$. If the concentration of the reactant after $30 \ minutes$ is $0.05 \ mol \ m^{-3}$,then its initial concentration will be ....... $mol \ m^{-3}$.

For a zero-order reaction,the correct expression for rate constant $(k)$ at half-life time $(t_{1/2})$ is ($[R_0] =$ initial concentration of reactant).

$A$ zero order reaction has a half-life time of $0.2 \ min$. If the initial concentration of the reactant is $0.2 \ mol \ dm^{-3}$,find the rate constant.