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

Intro to Chemical Equilibrium

General Chemistry

16. Chemical Equilibrium

Intro to Chemical Equilibrium

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Multiple Choice

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: 2 HBr(g) ⇌ H2(g) + Br2(g). At a certain temperature, a 2.00 L flask is initially filled only with 0.600 mol of HBr. If the equilibrium concentration of H2 is 0.100 M, what is the value of Kc at that temperature?

0.050

0.100

0.025

0.200

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Verified step by step guidance

Start by writing the balanced chemical equation for the decomposition of hydrogen bromide: 2 HBr(g) ⇌ H2(g) + Br2(g).

Identify the initial concentrations. Initially, the flask contains 0.600 mol of HBr in a 2.00 L flask, so the initial concentration of HBr is 0.600 mol / 2.00 L = 0.300 M. The initial concentrations of H2 and Br2 are both 0 M.

Determine the change in concentration at equilibrium. Since the equilibrium concentration of H2 is given as 0.100 M, and the stoichiometry of the reaction shows that 1 mol of H2 is produced for every 2 mol of HBr decomposed, the change in concentration of HBr is 2 times the change in H2, which is 0.200 M.

Calculate the equilibrium concentrations. The equilibrium concentration of HBr is the initial concentration minus the change: 0.300 M - 0.200 M = 0.100 M. The equilibrium concentration of Br2 is the same as H2, which is 0.100 M.

Use the equilibrium concentrations to calculate the equilibrium constant Kc. The expression for Kc is: Kc = ([H2][Br2]) / ([HBr]^2). Substitute the equilibrium concentrations into this expression to find the value of Kc.