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Electrolysis From Wikipedia, the free encyclopedia. Jump to: navigation, search 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. The most common form of electrolysis is electrolysis of water:

2H2O(l) → 2H2(g) + O2(g) Contents [hide] 1 Overview 2 Electrolysis of water 3 Experimenters 4 First law of electrolysis 5 Second law of electrolysis 6 Industrial uses 7 Domestic uses 8 Military uses 9 See also

[edit] 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. For example, when water is electrolyzed, hydrogen gas (H2) bubbles at the cathode, and oxygen gas (O2) rises at the anode. This effect was first discovered by William Nicholson, an English chemist, in 1800.

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. [edit] Electrolysis of water Main article: Electrolysis of water

One important use of electrolysis is to produce hydrogen. 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 is run into a cup of water. Hydrogen gas will be seen to bubble up at one of the immersed battery probes, and oxygen will bubble at the other.

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]

[edit] 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.

[edit] 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 current passed through the circuit. This became the basis of the first law of electrolysis.

[edit] 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.

[edit] Industrial uses Manufacture of aluminium, lithium, 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. [edit] Domestic uses Commerically available water ionizers use electrolysis to purify drinking water for in-home use. These units use titanium plates coated with platinum that act as an anode and cathode during the electrolysis of water. Two types of water are produced during electrolysis, acid and alkaline. Depending on the amount of dissolved solids contained in the source water, most residential counter top units can produce a range between 3.5pH to 11pH using municiple tap water. Peer reviewed clinical studies suggests that alkaline ionized water acts as an antioxidant by scavenging for active oxygen species. Domestic water ionizers produce water with redox values between -200 to -800 mV. Chlorine and sodium hydroxide are extracted from sodium chloride brine by electrolysis. Chlorine is, among many things, used as a disinfectant and for bleaching. Sodium hydroxide, or lye, is a strong base that is commonly used in drain cleaners.

[edit] 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 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.

[edit] See also Faraday's law of electrolysis The Faraday constant Michael Faraday Retrieved from "http://en.wikipedia.org/wiki/Electrolysis" Categories: Electrochemistry | Chemical processes | Electrolysis | Industrial processes

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if you are reading, you are so pathetic, you have far to much free time if you are able to read all of this!!!!! Get a kife

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