Thermodynamics & Electrochemistry

Flashcards covering key concepts from thermodynamics and electrochemistry.

Chemical Thermodynamics

The study of how heat and work are involved in chemical reactions and physical changes.

Spontaneous Process

A process that occurs under indicated conditions without external influence.

Nonspontaneous Process

A process that does not occur under the indicated conditions.

First Law of Thermodynamics

The total energy of the universe (system + surroundings) is constant; energy cannot be created or destroyed, only transformed.

Entropy (S)

A measure of the degree of disorder or randomness in a system.

Second Law of Thermodynamics

Spontaneous processes result in an overall increase in entropy of the universe.

Standard Molar Entropy (S°)

The entropy of 1 mole of a pure substance at 1 atm pressure, 1 M [solute] and 25°C (298 K).

Free Energy Change (ΔG)

The change in Gibbs free energy, calculated using enthalpy and entropy changes.

Exothermic Process

A process that releases heat to the surroundings.

Endothermic Process

A process that absorbs heat from the surroundings.

Gibbs Free Energy

A thermodynamic potential used to predict the spontaneity of a process.

Boltzmann's Equation

S = k ln W, where S is entropy, k is the Boltzmann constant, and W is the number of microstates.

Equilibrium Constant (K)

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

Oxidation

The process of losing electrons in a redox reaction.

Reduction

The process of gaining electrons in a redox reaction.

Oxidizing Agent

The substance that causes oxidation and is reduced in the process.

Reducing Agent

The substance that causes reduction and is oxidized in the process.

Nernst Equation

E = E° - RT/nF ln(Q), used to calculate cell potential under nonstandard conditions.