Free Energy and Thermodynamics Review

These flashcards cover key terminology and concepts related to free energy and thermodynamics, essential for understanding the principles of energy exchange and spontaneity in chemical processes.

First Law of Thermodynamics

Energy cannot be created or destroyed, only transformed.

Second Law of Thermodynamics

Energy tends to spread out and dissipate; entropy of the universe always increases.

Spontaneous Process

A process that occurs without ongoing outside intervention.

Nonspontaneous Process

A process that requires energy input to occur.

Entropy (S)

A thermodynamic function that increases with the number of energetically equivalent ways to arrange components of a system.

Gibbs Free Energy (G)

The maximum amount of work energy that can be released to the surroundings by a system at constant temperature and pressure.

Exothermic Process

A process that releases energy, often as heat.

Endothermic Process

A process that absorbs energy.

Microstate

The exact internal energy distribution among the particles at any one instant.

Macrostate

The state defined by a given set of measurable conditions (e.g., pressure, volume, temperature).

Heat Transfer

The process of thermal energy moving from one object to another.

Temperature Dependence of Entropy

Entropy change in surroundings is greater when heat is added at lower temperatures than at higher temperatures.

Standard Entropy (S°)

The entropy of 1 mole of a substance at 298 K under standard conditions.

Entropy Change (ΔS)

The difference in entropy between reactants and products during a reaction.

Free Energy Change (ΔG)

Indicator of spontaneity of a reaction; a negative ΔG indicates a spontaneous process.

Le Châtelier's Principle

The position of equilibrium shifts in response to changes in concentration, pressure, or temperature.

Equilibrium Constant (K)

A ratio of the concentrations of products to reactants at equilibrium.