| 1010 - Gibbs Free Energy |
| 1010 - Provide the definition for Gibbs Free Energy (ΔG = ΔH - TΔS) |
| 1015 - Understand Gibbs energy (ΔG) is the available (free) energy that can be applied to work. |
| 1020 - Use qualitative changes in enthalpy and entropy to predict the spontaneity of a process. |
| 1030 - Identify and give examples of systems that are spontaneous always, never, and only at either high or low temperatures. |
| 1040 - Know that if ΔG < 0 the process is spontaneous, and if ΔG > 0 it is not spontaneous (in the forward direction). |
| 1020 - delta S & delta G of Rxn |
| 1010 - Define and explain standard conditions. |
| 1020 - Use standard entropies to calculate the standard entropy change (ΔS˚) for a chemical reaction. |
| 1030 - State entropy is zero for a perfect crystal at absolute zero temperature. THIRD LAW |
| 1040 - Relate standard molar entropy to physical state, molar mass, atomic arrangement and molecular complexity. |
| 1050 - Use ΔS˚ and ΔH˚ of reaction to determine ΔG˚ (and thereby determine spontaneity). |
| 1030 - Non-Standard & Equilibrium |
| 1010 - Understand most chemical reactions do not occur under standard conditions. |
| 1020 - Solve for ΔG under non-standard conditions (ΔG = ΔG˚ + RT ln Q) |
| 1030 - Recognize that if a system is at equilibrium, ΔG = 0. |
| 1040 - Relate K to standard ΔG˚ and interconvert between them (ΔG˚ = - RT ln K ) |
| 1050 - For a standard system that is spontaneous, realize ΔG˚ < 0 and is therefore K > 1. |
| 1060 - For a standard system that is not spontaneous, realize ΔG˚ > 0 and is therefore K < 1. |
| 1070 - For a standard system that has a ΔG˚ = 0, realize this system is at equilibrium and K = 1. |