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

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Multiple Choice

Given the equilibrium reactions:A(g) + B2(g) <==> AB(g) + B(g) with KC = 4AB(g) <==> A(g) + B(g) with KC = 0.5What is the equilibrium constant (KC) for the following reaction?2A(g) + B2(g) <==> 2AB(g)

0.25

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Verified step by step guidance

Identify the given reactions and their equilibrium constants: Reaction 1: A(g) + B2(g) ⇌ AB(g) + B(g) with Kc1 = 4, Reaction 2: AB(g) ⇌ A(g) + B(g) with Kc2 = 0.5.

Recognize that the target reaction is 2A(g) + B2(g) ⇌ 2AB(g). This is a combination of the given reactions.

To find the equilibrium constant for the target reaction, manipulate the given reactions. Notice that the target reaction can be obtained by reversing Reaction 2 and then adding it to Reaction 1.

Reverse Reaction 2: A(g) + B(g) ⇌ AB(g). The equilibrium constant for the reversed reaction is the reciprocal of Kc2, which is 1/0.5 = 2.

Add the modified Reaction 2 to Reaction 1: (A(g) + B2(g) ⇌ AB(g) + B(g)) + (A(g) + B(g) ⇌ AB(g)) results in 2A(g) + B2(g) ⇌ 2AB(g). The equilibrium constant for the combined reaction is the product of the equilibrium constants of the individual reactions: Kc = Kc1 * (1/Kc2) = 4 * 2.