CH 112: Electrochemical Cells and Potential

Flashcards covering key concepts from Electrochemical Cells and Potential lecture.

Electrochemistry

The branch of chemistry that examines the transformations between chemical and electrical energy.

Redox reactions

Reactions involving a reduction half-reaction (gain of electrons) and an oxidation half-reaction (loss of electrons), which occur simultaneously.

Oxidation

A half-reaction where a reactant loses electrons.

Reduction

A half-reaction where a reactant gains electrons.

Electrochemical Cell

A device that converts chemical energy into electrical work, or vice versa.

Voltaic Cell

An electrochemical cell that transforms chemical energy into electrical energy by a spontaneous redox reaction.

Anode

The electrode at which the oxidation half-reaction occurs.

Cathode

The electrode at which the reduction half-reaction occurs.

Salt Bridge

A component of an electrochemical cell that connects the two solutions, balancing the flow of electrons.

Standard Reduction Potential (E°)

The potential of a half-reaction in standard state conditions (25°C, 1 M for solutes).

Standard Cell Potential (E° cell)

A measure of how forcefully an electrochemical cell can pump electrons through an external circuit.

Nernst Equation

An equation that relates the cell potential to the standard cell potential and the reaction quotient.

Corrosion

The process by which a metal is oxidized by substances in its environment.

Electrolytic Cell

An electrochemical cell where electrical energy drives a nonspontaneous reaction.

Sacrificial Anode

A technique used in cathodic protection to prevent corrosion of a metal structure.

Faraday's Constant (F)

The amount of electric charge per mole of electrons, approximately 96,485 C/mol.

Voltage

The electric potential difference between two points, measured in volts.

Work (electrical)

The energy produced by an electrochemical cell, often calculated as welec = -CEcell.