---
title: "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?"
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url: "https://nerd-notes.com/ubq/123780/"
date_modified: "2026-09-28T12:30:17+00:00"
---

# 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?

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?

- **A.** Reaction III \(>\) Reaction II \(>\) Reaction I
- **B.** Reaction III \(>\) Reaction I \(>\) Reaction II
- **C.** Reaction I \(>\) Reaction II \(>\) Reaction III
- **D.** Reaction I \(>\) Reaction III \(>\) Reaction II

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123780/*