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This article is about the chemical process. Electrolysis is also a method of depilation.

In chemistry and manufacturing, electrolysis is a method of separating bonded elements and compounds by passing an electric current through them.

1 Overview
2 Electrolysis of water
3 Experimenters
4 First law of electrolysis
5 Second law of electrolysis
6 Industrial uses
7 Military uses
8 Examples
9 See also

Overview

An ionic compound is dissolved with an appropriate solvent, or otherwise melted by heat, so that its ions are available in the liquid. An electrical current is applied between a pair of metal electrodes immersed in the liquid. The negatively charged electrode is called the cathode, and the positively charged one the anode. Each electrode attracts ions which are of the opposite charge. Therefore, positively charged ions (called cations) move towards the cathode, while negatively charged ions (termed anions) move toward the anode. The energy required to separate the ions, and cause them to gather at the respective electrodes, is provided by an electrical power supply. At the probes, electrons are absorbed or released by the ions, forming a collection of the desired element or compound.

The amount of electrical energy that must be added equals the change in Gibbs free energy of the reaction plus the losses in the system. The losses can (theoretically) be arbitrarily close to zero, so the maximum thermodynamic efficiency equals the enthalpy change divided by the free energy change of the reaction. In most cases the electric input is larger than the enthalpy change of the reaction, so some energy is released in the form of heat. In some cases, for instance in the electrolysis of steam into hydrogen and oxygen at high temperature, the opposite is true. Heat is absorbed from the surroundings, and the heating value of the produced hydrogen is higher than the electric input. In this case the efficiency can be said to be greater than 100%. (It is worth noting that the maximum theoretic efficiency of a fuel cell is the inverse of that of electrolysis. It is thus impossible to create a perpetual motion machine by combining the two processes. See water fuel cell for an example of such an attempt.)

The following technologies are related to electrolysis:

Electrochemical cells, including the hydrogen fuel cell, use the reverse of this process.
Gel electrophoresis is an electrolysis where the solvent is a gel: it is used to separate substances, such as DNA strands, based on their electrical charge.

Electrolysis of water

Main article: Electrolysis of water

One important use of electrolysis is to produce hydrogen. The reaction that occurs is

2H₂O_(aq) → 2H_2(g) + O_2(g)

In the future, this could play a central role in shifting our society over to a reliance on hydrogen as an energy carrier for powering electric motors and internal combustion engines. (See hydrogen economy.) Electrolysis of water can be achieved in a simple hands-on project, where electricity from a battery or low voltage DC power supply (eg computer power supply 5v rail) is run into a cup of water (in practice a saltwater solution or other electrolyte will need to be used otherwise no result will be observed). Using platinum electrodes, hydrogen gas will be seen to bubble up at the cathode, and oxygen will bubble at the anode. Using any other electrode for the anode however, the oxygen will react with the anode instead of being released as a gas. For example using iron electrodes in a sodium chloride solution electrolyte, iron oxide will be produced at the anode, which will react to form iron hydroxide. When producing large quantites of hydrogen, this can significantly gunge up the electrolytic cell - which is why iron is not used for commercial electrolysis.

The energy efficiency of water electrolysis varies widely. Some report 50–70%[1], while others report 80–94%.[2] These values only refer to the efficiency of converting electrical energy into hydrogen's chemical energy. The energy lost in generating the electricity is not included. For instance, when considering a power plant that converts the heat of nuclear reactions into hydrogen via electrolysis, the total efficiency is more like 25–40%.[3]

Experimenters

Scientific pioneers of electrolysis included:

Humphry Davy
Michael Faraday
Paul Héroult
Svante Arrhenius
Adolph Wilhelm Hermann Kolbe

More recently, electrolysis of heavy water was performed by Fleischmann and Pons in their famous experiment, resulting in anomalous heat generation and the controversial claim of cold fusion.

First law of electrolysis

In 1832, Michael Faraday reported that the quantity of elements separated by passing an electrical current through a molten or dissolved salt was proportional to the quantity of electric charge passed through the circuit. This became the basis of the first law of electrolysis.

Second law of electrolysis

Faraday also discovered that the mass of the resulting separated elements was directly proportional to the atomic masses of the elements when an appropriate integral divisor was applied. This provided strong evidence that discrete particles of electricity existed as parts of the atoms of elements.

Industrial uses

Manufacture of aluminium, lithium, sodium, potassium, aspirin.
Manufacture of hydrogen for hydrogen cars and fuel cells.
High-temperature electrolysis is also being used for this.
Coulometric techniques can be used to determine the amount of matter transformed during electrolysis by measuring the amount of electricity required to perform the electrolysis.
Manufacture of chlorine and sodium hydroxide.
Manufacture of sodium and potassium chlorate.
Manufacture of perfluorinated organic compounds like trifluoroacetic acid.

Military uses

As well as producing hydrogen, electrolysis also produces oxygen. Nuclear submarines are able to generate breathing oxygen from the water around them. This enables submarines to stay underwater for an indefinite period of time.

Space Stations can also use electrolysis to produce amounts of extra oxygen from waste water or surplus water produced from the Space Shuttle fuel cells.

Both these applications depend on having an abundant electrical supply, either from the reactor or solar panels.

Examples

Electrolysis of an aqueous solution of table salt (NaCl, or sodium chloride) produces aqueous sodium hydroxide and chlorine. In practice this only occurs in exceptional circumstances. NaCl(aq) can be reliably electrolysed to produce hydrogen. In order to produce chlorine in a commercial situation, molten sodium chloride is electrolysed to produce sodium metal and chlorine gas. These will react violently, so a Mercury Cell is used to ensure they do not come into contact with each other.

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This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "electrolysis".