Electrochemistry Fundamentals

This lecture covers the fundamentals of electrochemistry, focusing on cell potential, current production, and the relationship between current and reactant conversion. It explains the concepts of standard cell potential, equilibrium potential, and open circuit potential. The instructor discusses the effect of electrode material and additional electrolytes on current-voltage plots, emphasizing the importance of overpotential in driving reactions. Analogies between chemical reactivity and electrochemistry are explored, highlighting the role of overpotential in reaction rates. The lecture concludes with a discussion on deriving analytical expressions for current-voltage curves.

About this result

This page is automatically generated and may contain information that is not correct, complete, up-to-date, or relevant to your search query. The same applies to every other page on this website. Please make sure to verify the information with EPFL's official sources.

Related lectures (219)

Related concepts (242)

ChE-407: Electrochemical engineering

This course builds upon the underlying theory in thermodynamics, reaction kinetics, and transport and applies these methods to electrosynthesis, fuel cell, and battery applications. Special focus is p

Standard electrode potential

In electrochemistry, standard electrode potential , or , is a measure of the reducing power of any element or compound. The IUPAC "Gold Book" defines it as: "the value of the standard emf (electromotive force) of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode". The basis for an electrochemical cell, such as the galvanic cell, is always a redox reaction which can be broken down into two half-reactions: oxidation at anode (loss of electron) and reduction at cathode (gain of electron).

Reduction potential

Redox potential (also known as oxidation / reduction potential, ORP, pe, , or ) is a measure of the tendency of a chemical species to acquire electrons from or lose electrons to an electrode and thereby be reduced or oxidised respectively. Redox potential is expressed in volts (V). Each species has its own intrinsic redox potential; for example, the more positive the reduction potential (reduction potential is more often used due to general formalism in electrochemistry), the greater the species' affinity for electrons and tendency to be reduced.

Membrane potential

Membrane potential (also transmembrane potential or membrane voltage) is the difference in electric potential between the interior and the exterior of a biological cell. That is, there is a difference in the energy required for electric charges to move from the internal to exterior cellular environments and vice versa, as long as there is no acquisition of kinetic energy or the production of radiation. The concentration gradients of the charges directly determine this energy requirement.

Electrode potential

In electrochemistry, electrode potential is the electromotive force of a galvanic cell built from a standard reference electrode and another electrode to be characterized. By convention, the reference electrode is the standard hydrogen electrode (SHE). It is defined to have a potential of zero volts. It may also be defined as the potential difference between the charged metallic rods and salt solution. The electrode potential has its origin in the potential difference developed at the interface between the electrode and the electrolyte.

Electrochemical cell

An electrochemical cell is a device that generates electrical energy from chemical reactions. Electrical energy can also be applied to these cells to cause chemical reactions to occur. Electrochemical cells which generate an electric current are called voltaic or galvanic cells and those that generate chemical reactions, via electrolysis for example, are called electrolytic cells. Both galvanic and electrolytic cells can be thought of as having two half-cells: consisting of separate oxidation and reduction reactions.

Solar Energy Conversion Devices ME-468: Solar energy conversion

Explores solar energy conversion devices, electrochemistry, efficiency calculations, and mass transfer modes in solar energy systems.

Electrochemical Cell: pH Calculation CH-160(en): Advanced general chemistry (english)

Covers the calculation of pH in an electrochemical cell scenario involving copper and hydrogen electrodes.

Redox Reactions: Half-Reactions, Potentials, and Applications MSE-101(a): Materials:from chemistry to properties

Explores redox reactions, electrode potentials, and their practical uses in electrochemistry.

Electrochemical Thermodynamics: Efficiency and Potentials ChE-407: Electrochemical engineering

Explores electrochemical thermodynamics, efficiency, potentials, and their practical applications in fuel cells and non-standard conditions.

Dynamic Electrochemistry: Butler-Volmer Equation CH-341: Physical chemistry of interfaces

Explores the Butler-Volmer equation and its role in electrochemistry applications.