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 K

General Chemistry

16. Chemical Equilibrium

Equilibrium Constant K

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

At a certain temperature, the equilibrium constant Kc for the reaction 2 C(s) + O2(g) ⇌ 2 CO(g) is 4.72. What is the equilibrium constant Kc for the reverse reaction CO(g) ⇌ C(s) + 0.5 O2(g) at the same temperature?

9.44

2.36

0.212

4.72

Previous problemNext problem

Verified step by step guidance

Understand that the equilibrium constant (Kc) for a reaction is related to the concentrations of the products and reactants at equilibrium. For the given reaction, 2 C(s) + O2(g) ⇌ 2 CO(g), the Kc is 4.72.

Recognize that reversing a chemical reaction involves inverting the equilibrium constant. If the forward reaction has an equilibrium constant Kc, the reverse reaction will have an equilibrium constant of 1/Kc.

Write the expression for the reverse reaction: CO(g) ⇌ C(s) + 0.5 O2(g). Note that the stoichiometry of the reverse reaction is different from the forward reaction.

Calculate the equilibrium constant for the reverse reaction by taking the reciprocal of the Kc for the forward reaction. Use the formula: Kc(reverse) = 1/Kc(forward).

Substitute the given Kc value for the forward reaction into the formula: Kc(reverse) = 1/4.72. This will give you the equilibrium constant for the reverse reaction.