Electrochemistry Foundations Flashcards

A comprehensive set of vocabulary flashcards covering the fundamental principles of electrochemistry, cell components, thermodynamics, and stoichiometry as discussed in the lecture.

Voltaic Cell

Also known as a galvanic cell, it is an electrochemical cell that produces energy through a spontaneous reaction with a positive cell potential.

Electrolytic Cell

An electrochemical cell that consumes energy from an outside source to drive a reaction forward, where the cell potential can be positive or negative.

Oxidation

A process where a substance loses electrons, resulting in an increase in its oxidation state.

Reduction

A process where a substance gains electrons, resulting in a decrease or reduction of its oxidation state.

Anode

The electrode where oxidation occurs; electrons always flow from this electrode to the cathode, and it typically loses mass.

Cathode

The electrode where reduction occurs; electrons flow toward this electrode, and it typically gains mass as ions deposit onto it.

Salt Bridge

A component of an electrochemical cell that maintains charge balance by allowing cations to travel toward the cathode and anions to travel toward the anode.

Standard Cell Potential ($E^\circ$)

The potential of a cell measured under standard conditions, where ion concentrations are exactly $1\,\text{mol/liter}$.

Oxidizing Agent

The reactant that is reduced in a redox reaction, thereby causing the oxidation of another substance.

Reducing Agent

The reactant that is oxidized in a redox reaction, thereby causing the reduction of another substance.

Gibbs Free Energy ($\Delta G$)

The measure of the maximum electrical work a cell can perform, calculated using the equation $\Delta G = -nFE$.

Faraday's Constant ($F$)

A constant value representing the charge of one mole of electrons, approximately equal to $96,485\,\text{C/mol } e^-$.

Volt ($V$)

A unit of electrical potential defined as one joule of energy per one coulomb of charge ($1\,\text{J/C}$).

Nernst Equation

An equation used to calculate the cell potential under non-standard conditions: $E = E^\circ - \frac{0.0591}{n} \log(Q)$.

Reaction Quotient ($Q$)

The ratio of the initial concentrations of products to reactants, excluding solids and liquids, used to determine the direction of a reaction.

Ampere (Amp)

A unit of electric current where one coulomb of charge is equal to one amp times one second ($1\,\text{C} = 1\,\text{A} \times 1\,\text{s}$).

Inert Electrode

A non-reactive electrode material, such as platinum ($Pt$), palladium ($Pd$), or carbon graphite, used when the half-reaction does not involve a solid metal.

Equilibrium Constant ($K$)

A value that relates to $\Delta G^\circ$ via the equation $\Delta G^\circ = -RT \ln(K)$; if K > 1, the reaction is product-favored at equilibrium.