Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

16. Chemical Equilibrium

Equilibrium Constant Calculations

General Chemistry

16. Chemical Equilibrium

Equilibrium Constant Calculations

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9. If Kc = 0.143 at 25°C for this reaction and the initial concentration of C6H12 is 1.0 M with no CH3C5H9 present initially, what are the equilibrium concentrations of C6H12 and CH3C5H9?

[C6H12] = 0.875 M, [CH3C5H9] = 0.125 M

[C6H12] = 0.900 M, [CH3C5H9] = 0.100 M

[C6H12] = 0.800 M, [CH3C5H9] = 0.200 M

[C6H12] = 0.857 M, [CH3C5H9] = 0.143 M

Previous problemNext problem

Verified step by step guidance

Start by writing the balanced chemical equation for the reaction: \( \text{C}_6\text{H}_{12} \rightleftharpoons \text{CH}_3\text{C}_5\text{H}_9 \).

Define the initial concentrations: \([\text{C}_6\text{H}_{12}] = 1.0 \text{ M}\) and \([\text{CH}_3\text{C}_5\text{H}_9] = 0 \text{ M}\).

Set up an ICE table (Initial, Change, Equilibrium) to track the changes in concentration. Let \(x\) be the change in concentration of \(\text{CH}_3\text{C}_5\text{H}_9\) formed at equilibrium.

Write the expression for the equilibrium constant \(K_c\): \(K_c = \frac{[\text{CH}_3\text{C}_5\text{H}_9]}{[\text{C}_6\text{H}_{12}]}\). Substitute the equilibrium concentrations from the ICE table into this expression.

Solve the equation \(0.143 = \frac{x}{1.0 - x}\) for \(x\) to find the equilibrium concentrations of \([\text{C}_6\text{H}_{12}]\) and \([\text{CH}_3\text{C}_5\text{H}_9]\).