228- Considering the graph below, which of the following statements about the related reaction is correct? [Figure: A concentration vs. reaction progress graph showing three curves labeled a, b, and c. Curve a starts at 0.6 and decreases, curve b starts at 0.5 and decreases, and curve c starts near 0 and increases, all reaching equilibrium. The y-axis is labeled $\mathrm{mol \cdot L^{-1}}$ with values 0.1 through 0.6, and the x-axis is labeled reaction progress.]
[A)] The equilibrium constant of this reaction under experimental conditions is $0.5\ \mathrm{L.mol^{-1}}$.
[B)] a, b, and c can be $\mathrm{H_2(g)}$, $\mathrm{I_2(g)}$, and $\mathrm{HI(g)}$, respectively.
[P)] It can correspond to the reaction: $\mathrm{2NO(g) + Cl_2(g) \rightleftharpoons 2NOCl(g)}$, which is reversible.
[T)] It can be related to the reaction: $\mathrm{COCl_2(g) \rightleftharpoons CO(g) + Cl_2(g)}$, giving a ratio.
(1) A, P (2) A, B (3) B, T (4) P, T
\textbf{228-} Considering the graph below, which of the following statements about the related reaction is correct?
\textit{[Figure: A concentration vs. reaction progress graph showing three curves labeled a, b, and c. Curve a starts at 0.6 and decreases, curve b starts at 0.5 and decreases, and curve c starts near 0 and increases, all reaching equilibrium. The y-axis is labeled $\mathrm{mol \cdot L^{-1}}$ with values 0.1 through 0.6, and the x-axis is labeled reaction progress.]}
\begin{itemize}
\item[A)] The equilibrium constant of this reaction under experimental conditions is $0.5\ \mathrm{L.mol^{-1}}$.
\item[B)] a, b, and c can be $\mathrm{H_2(g)}$, $\mathrm{I_2(g)}$, and $\mathrm{HI(g)}$, respectively.
\item[P)] It can correspond to the reaction: $\mathrm{2NO(g) + Cl_2(g) \rightleftharpoons 2NOCl(g)}$, which is reversible.
\item[T)] It can be related to the reaction: $\mathrm{COCl_2(g) \rightleftharpoons CO(g) + Cl_2(g)}$, giving a ratio.
\end{itemize}
(1) A, P \quad (2) A, B \quad (3) B, T \quad (4) P, T