Three separate rigid \(1.0\text{ L}\) vessels at \(298\text{ K}\) initially contain \(1.0\text{ mol}\) of \(\text{AB}(g)\), \(\text{CD}(g)\), and \(\text{EF}(g)\), respectively. The three gases decompose according to the reactions and equilibrium constants shown in the table below.

Reaction	Equation	Equilibrium Constant, \(K_c\)
I	\(\text{AB}(g) \rightleftharpoons \text{A}(g) + \text{B}(g)\)	\(4.0 \times 10^{-12}\)
II	\(\text{CD}(g) \rightleftharpoons \text{C}(g) + \text{D}(g)\)	\(1.5 \times 10^{-2}\)
III	\(\text{EF}(g) \rightleftharpoons \text{E}(g) + \text{F}(g)\)	\(8.0 \times 10^{6}\)

Which of the following correctly ranks the reactions in order of the percent of initial reactant converted to products once equilibrium is established, from greatest to least?