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

19. Chemical Thermodynamics

Gibbs Free Energy Calculations

General Chemistry

19. Chemical Thermodynamics

Gibbs Free Energy Calculations

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Multiple Choice

Gibbs free energy is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction and is minimized at equilibrium. The change in Gibbs free energy can be calculated by ΔG°_rxn = ΔH°_rxn - TΔS°_rxn where ΔG°_rxn is:

the standard enthalpy change of the reaction

the standard entropy change of the reaction

the standard Gibbs free energy change of the reaction

the equilibrium constant of the reaction

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Verified step by step guidance

Begin by understanding the Gibbs free energy equation: ΔG°_rxn = ΔH°_rxn - TΔS°_rxn. This equation relates the change in Gibbs free energy (ΔG°_rxn) to the change in enthalpy (ΔH°_rxn), temperature (T), and change in entropy (ΔS°_rxn).

Identify each term in the equation: ΔG°_rxn represents the standard Gibbs free energy change of the reaction, ΔH°_rxn is the standard enthalpy change, T is the temperature in Kelvin, and ΔS°_rxn is the standard entropy change.

Recognize that the Gibbs free energy change (ΔG°_rxn) indicates the spontaneity of a reaction. A negative ΔG°_rxn suggests that the reaction is spontaneous under standard conditions.

Understand that at equilibrium, the Gibbs free energy is minimized, meaning ΔG°_rxn approaches zero, and the reaction is at a state where the forward and reverse reactions occur at the same rate.

Relate the Gibbs free energy change to the equilibrium constant (K) using the equation ΔG°_rxn = -RT ln(K), where R is the universal gas constant and T is the temperature. This shows how Gibbs free energy is connected to the equilibrium constant of the reaction.