Lecture

Battery Diagram and Electrode Reactions

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In course

CH-160(b): General chemistry

Cet enseignement vise l'acquisition des notions essentielles relatives à la structure de la matière, aux équilibres et à la réactivité chimiques. Le cours et les exercices fournissent la méthodologie permettant de résoudre par le raisonnement et le calcul ...

Description

This lecture covers the construction of a battery with two electrodes connected by a salt bridge. It discusses the polarity of the electrodes, the potential difference, and the reactions at each electrode, including the global spontaneous reaction. The lecture also involves calculating the pH and pKa of specific solutions, such as ammonium chloride and iron sulfate. Various concepts related to electrochemistry and redox reactions are explored in detail.

Instructor

Samuel Terrettaz

Teaching & PhD Courses Advanced general chemistry CH-160(f) This course aims at the acquisition of essential notions on the structure of matter, chemical equilibria and reactivity. Theoretical teaching and exercise provide the methodology to analyze and solve by reasoning and calculation novel problems of general chemistry. Advanced general chemistry CH-160(g) This course aims at the acquisition of essential notions on the structure of matter, chemical equilibria and reactivi

Official source

Ontological neighbourhood

Chemistry

Physical chemistry: Electrochemistry

Related concepts (32)

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.

Electrode

An electrode is an electrical conductor used to make contact with a nonmetallic part of a circuit (e.g. a semiconductor, an electrolyte, a vacuum or air). Electrodes are essential parts of batteries that can consist of a variety of materials depending on the type of battery. The electrophore, invented by Johan Wilcke, was an early version of an electrode used to study static electricity. Electrodes are an essential part of any battery. The first electrochemical battery made was devised by Alessandro Volta and was aptly named the Voltaic cell.

Reference electrode

A reference electrode is an electrode that has a stable and well-known electrode potential. The overall chemical reaction taking place in a cell is made up of two independent half-reactions, which describe chemical changes at the two electrodes. To focus on the reaction at the working electrode, the reference electrode is standardized with constant (buffered or saturated) concentrations of each participant of the redox reaction. There are many ways reference electrodes are used.

Standard hydrogen electrode

In electrochemistry, the standard hydrogen electrode (abbreviated SHE), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials. Its absolute electrode potential is estimated to be 4.44 ± 0.02 V at 25 °C, but to form a basis for comparison with all other electrochemical reactions, hydrogen's standard electrode potential (E°) is declared to be zero volts at any temperature. Potentials of all other electrodes are compared with that of the standard hydrogen electrode at the same temperature.

Volta potential

The Volta potential (also called Volta potential difference, contact potential difference, outer potential difference, Δψ, or "delta psi") in electrochemistry, is the electrostatic potential difference between two metals (or one metal and one electrolyte) that are in contact and are in thermodynamic equilibrium. Specifically, it is the potential difference between a point close to the surface of the first metal and a point close to the surface of the second metal (or electrolyte). The Volta potential is named after Alessandro Volta.

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