To solve this problem, we need to understand the graphical representation of zero-order and first-order reactions.$\newline$The graph provided shows a constant line, which is characteristic of a zero-order reaction.$\newline$For zero-order reactions:$\newline •$The rate of reaction is independent of the concentration of the reactant.$\newline •$The concentration of the reactant decreases linearly with time.$\newline •$Thus, a plot of concentration vs. time is a straight line.$\newline$For first-order reactions:$\newline •$The rate of reaction is directly proportional to the concentration of the reactant.$\newline •$The half-life $(t_{1/2})$ is constant and independent of the initial concentration.$\newline •$A plot of $t_{1/2}$ vs. concentration is a horizontal line.$\newline$Analyzing the options:$\newline$Option 1: Zero order: $(y =$concentration$, x =$time$),$ First order: $(y = t_{1/2}, x =$concentration$) \newline$Option 2: Zero order: $(y =$concentration$, x =$time$),$ First order: $(y =$rate constant$, x =$concentration$) \newline$Option 3: Zero order: $(y =$rate$, x =$concentration$),$ First order: $(y = t_{1/2}, x =$concentration$) \newline$Option 4: Zero order: $(y =$rate$, x =$concentration$),$ First order: $(y =$rate$, x = t_{1/2}) \newline$The correct representation for the graph is:$\newline$Zero order: $(y =$rate$, x =$concentration$),$ First order: $(y = t_{1/2}, x =$concentration$) \newline$This corresponds to Option 3.