The rate constant for a zero order reaction $A \rightarrow$ products is $0.0030 \ mol \ L^{-1} \ s^{-1}$. How long will it take for the initial concentration of $A$ to fall from $0.10 \ M$ to $0.075 \ M$ (in $s$)?

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

If the slope of a line of the graph between dissociated concentration of reactant $([A]_0 - [A]_t)$ and time ($t$ in $min$) for a zero order reaction is $0.02 \ mol \ L^{-1} \ min^{-1}$,then calculate the initial concentration of reactant $([A]_0)$,if after $30 \ min$ its concentration $([A]_t)$ is $0.05 \ mol \ L^{-1}$. (in $M$)

The half-life of a zero-order reaction is $1 \text{ hour}$. If the initial concentration of the reactant is $2.0 \text{ mol L}^{-1}$, find the time required to decrease the concentration from $0.50 \text{ mol L}^{-1}$ to $0.25 \text{ mol L}^{-1}$. (in $\text{ hour}$)

Calculate the rate constant of a zero order reaction if it is $90 \%$ completed in $90 \ s$.

What is the unit for the zero order rate constant?