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 decomposition of $NH_3$ on a platinum surface is a zero-order reaction. What is the rate of production of $N_2$ if $k = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$?

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 ....... $M$.

The unit of rate constant for a zero order reaction is

$5$ milli-moles of a solid $A$ was dissolved in $5$ moles of $H_2O$. On adding to the solvent,$A$ starts polymerising into another insoluble solid following zero order kinetics. On adding $6$ milli-moles of another solid solute $C$ (after $20$ minutes) the polymerisation completely stops. The insoluble solid polymer is removed and the resulting solution was cooled to a temperature less than $-0.186\,^{\circ}C$ (melting point of solution) to cause solidification of some liquid water. Calculate the value of $'X'$ if rate constant for polymerisation reaction is represented as $10^{-X}\,moles/minute$. $[K_f(H_2O) = 1.86\, K\, Kg\,mol^{-1}]$

Which of the following is a zero order reaction?