Thermodynamics III Lecture Notes

Flashcards covering key vocabulary and concepts from Thermodynamics III lecture notes.

Helmholtz Energy (A)

Thermodynamic function; A ≡ U − TS

Gibbs Free Energy (G)

Thermodynamic function; G ≡ H − TS

ΔA (at constant V and T)

At constant V and T, ΔA = ΔU − TΔS ≤ 0

ΔG (at constant P and T)

At constant P and T, ΔG = ΔH − TΔS ≤ 0

ΔA (Maximum Work)

The most negative value of w, when a system is doing work to its surrounding

ΔG (Free Work)

Theoretical limit of how much free work can be done by a system at constant T and P

Standard Gibbs Free Energy of Formation (ΔGf o)

Gibbs free energy change for the formation of a mole of a compound from its constituted elements in their standard states (1.00 atm and 298.15 K)

Chemical Potential (µ)

ΔG per mole of quantity (Δn) change of a component in the mixture or reaction at constant T and P

Chemical Potential (µ) - Analogy

Molecules moves/migrates from high concentration to a low one.

Gibbs Free Energy of Mixing (ΔGmix)

The change in Gibbs free energy when mixing two or more substances.

Qp

Reaction quotient of pressure; conceptually identical to the equilibrium constant (Kp)

KP

Equilibrium constant expressed in terms of partial pressures.

Van't Hoff Equation

Describes the dependence of the equilibrium constant on temperature.

Maxwell Equations

Relationship between partial derivatives of thermodynamic properties.

πT

Internal pressure