For a zero order reaction $A \longrightarrow \text{product}$,consider the following graph:
Where $[A_t]$ is the remaining concentration of reactant $A$ at time $t$. Calculate the concentration of $A$ after $2 \ s$. (in $mol/L$)

What is the formula to find the value of $t_{1/2}$ for a Zero Order Reaction?

In the following reaction $A \to B + C,$ the rate constant is $0.001 \ M \ s^{-1}.$ If we start with $1 \ M$ of $A,$ then the concentrations of $A$ and $B$ after $10 \ minutes$ are respectively:

$5$ 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 graph represents a zero order reaction $[A_{(g)} \to B_{(g)}]$?

For a zero order reaction,which of the following statements is false?