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	Faraday's law - HighBeam Encyclopedia (Site not responding. Last check: 2007-11-02)
		Faraday's law physical law stating that the number of moles of substance produced at an electrode during electrolysis is directly proportional to the number of moles of electrons transferred at that electrode; the law is named for Michael Faraday, who formulated it in 1834.
		The number of faradays required to produce one mole of substance at an electrode depends upon the way in which the substance is oxidized or reduced (see oxidation and reduction).
		For example, in the electrolysis of molten sodium chloride, NaCl, one faraday, or one mole, of electrons is transferred at the cathode to one mole of sodium ions, Na, to form one mole of sodium atoms, Na, while in the electrolysis of molten magnesium chloride, MgCl
	www.encyclopedia.com /doc/1E1-faradays.html (300 words)

	Faradays Law: Free Encyclopedia Articles at Questia.com Online Library
		physical law stating that the number of moles of substance produced at an electrode during electrolysis is directly proportional to the number of moles of electrons transferred at that electrode; the law is named for Michael Faraday, who formulated it in 1834.
		It is the second law of thermodynamics that holds dominion over...organization of the universe, and what the law has to say we find verified by ordinary...
		FARADAYS LAW physical law stating that the number...electrons transferred at that electrode; the law is named for Michael Faraday, who formulated...equal to 96,500 coulombs.
	www.questia.com /library/encyclopedia/faradays-law.jsp?l=F&p=1 (1279 words)

	electrolysis superpage
		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.
		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.
		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.
	www.equityedu.com /Elec-to-Emac/electrolysis.php (1518 words)

	A Q U A R I U S (Site not responding. Last check: 2007-11-02)
		Electrolysis of water can be achieved in a simple hands-on project, where electricity from a battery is passed through a container of water (in practice a saltwater solution or other electrolyte will need to be used otherwise no result will be observed).
		The number of Faradays of electric charge required to discharge one mole of substance at an electrode is equal to the number of "excess" elementary charges on that ion.
		In real electrolysis systems, a different solution is used and higher levels of electricity help to split the water molecules into hydrogen and oxygen without this secondary reaction.
	www.bigelow.org /aquarius/electrolysis.html (2273 words)

	Continuous Electrodeionization - Faradys Law (Site not responding. Last check: 2007-11-02)
		Faraday's Law states that the electric charge required to liberate one gram-equivalent of a substance by electrolysis is 96,487 coulombs (a coulomb is the amount of electric charge that crosses a surface in one second when a steady current of one ampere is flowing across the surface).
		In both electrodialysis and electrodeionization, Faraday's Law is used to relate the transfer of salts through the membranes and the amount of current flowing through the membranes.
		Ohm's law states that the direct current flowing in an electric circuit is directly proportional to the voltage applied, and inversely proportional to the resistance of the element:
	www.cediuniversity.com /index-3c.html (754 words)

	Joseph's Diary (Site not responding. Last check: 2007-11-02)
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	Electrolysis
		Electrolysis involves passing an electric current through either a molten salt or an ionic solution.
		The ions are "forced" to undergo either oxidation (at the anode) or reduction (at the cathode).
		Most electrolysis problems are really stoichiometry problems with the addition of an amount of electric current.
	www.chem.purdue.edu /gchelp/howtosolveit/Electrochem/Electrolysis.htm (607 words)

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	Faradays law electrolysis (Site not responding. Last check: 2007-11-02)
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	Faraday's law — FactMonster.com
		is directly proportional to the number of moles of electrons transferred at that electrode; the law is named for Michael Faraday, who formulated it in 1834.
		The number of faradays required to produce one mole of substance at an electrode depends upon the way in which the substance is oxidized or reduced (see
		Michael Faraday - Faraday, Michael, 1791–1867, English scientist.
	www.factmonster.com /ce6/sci/A0818248.html (233 words)

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	Ideal gas law constants (Site not responding. Last check: 2007-11-02)
		Faradays law of electrolysis 8 ideal gas law constants.
		Recall the ideal gas law is. Table 3-1 Henry¡¯s Law Constants for CO ideal gas law constants.
		E. Faradays law of electrolysis ideal gas law constants.
	www.gas-resources.com /ideal-gas-law-constants.html (635 words)

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	AllRefer.com - Faraday's law (Chemistry) - Encyclopedia
		You are here : AllRefer.com > Reference > Encyclopedia > Chemistry, General > Faraday's law
		Topics that might be of interest to you:
		More articles from AllRefer Reference on Faraday's law
	reference.allrefer.com /encyclopedia/F/Faradays.html (273 words)

	Faraday constant - Wikipedia, the free encyclopedia
		In physics and chemistry, the Faraday constant is the amount of electric charge in one mole of electrons.
		The Faraday constant was named after British scientist Michael Faraday.
		It is used in electrolytic system calculations to determine the mass of a chemical species that will collect at an electrode.
	en.wikipedia.org /wiki/Faraday_constant (191 words)

	An Investigation Into The Factors Which Effect The Electrolysis Of Copper Sulphate Solution
		It is known that by passing a constant electric current through an aqueous copper sulphate solution that the passage of ions through this solution results in copper atoms being dissolved into the solution from the anode while positive copper ions (cations) being discharged at the cathode.
		This statement can be supported by both of Faraday’s Laws.
		“The mass of an element deposited by one Faraday of electricity is equal to the atomic mass in grams of the element divided by the number of electrons required to discharge one ion of the element.”
	www.courseworkhelp.co.uk /GCSE/Science/09.htm (1149 words)

	Page Three - CORE_Chapter Seventeen - Electrochemistry (Site not responding. Last check: 2007-11-02)
		This video shows the electrolysis of an aqueous solution of KI with graphite electrodes.
		This is the document for the microscale electrochemical cells lab.
		This is the document for the determination of the value of the faraday lab.
	www.dlt.ncssm.edu /core/c17-3.htm (144 words)

	Untitled Document
		The lesson books have been correlated to the California Science Standards, the National Science Education Standards, and the Benchmarks for Science Literacy.
		Determine the energy efficiency of a fuel cell using Faradays’ law of electrolysis.
		Determine the Avogadro Constant using an electrolyser or a fuel cell.
	www.solore.com.tw /power/fuel/educational/Solar-kit-1.htm (330 words)

	Electrolysis
		Enter the number seconds or hours of time that the substance will be produced/consumed at the electrode/anode.
		Enter the current in Amperes, and the time in either seconds or hours.
		Calculates the mass using molar mass of a substance or the volume of gas using the ideal gas law (PV = nRT) by selecting the option using the radio buttons.
	elgersmad.homestead.com /files/Calculators/Electrolysis.htm (545 words)

	Explain faradays law of electrolysis (Site not responding. Last check: 2007-11-02)
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	Faraday's law — Infoplease.com
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	9374. Factors that affect Faradays Law of electrolysis
		I am currently doing a project on Faradays Law of Electrolysis and I am desperatly trying to find out what conditions Faraday did the experiments under, and mainly what factors may affect the rate of consumption of the metals in the system.
		I know the current passing through the system affects the consumption rate, but I can't find any papers that tell of any other factors.
		I think that was Faraday's point: one Faraday of electricity (96,500 amp-seconds) deposits one gram molecular weight.
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	Solar Hydrogen Starter Kit (via CobWeb/3.1 planetlab2.tamu.edu) (Site not responding. Last check: 2007-11-02)
		Consumption of Distilled Water: 1ml/10h at 300 mA electrolysis current
		Amount of Water carried from oxygen to hydrogen side: 1ml/h at 500 mA electrolysis current
		Determine the energy efficiency of a fuel cell using Faradays?
	www.fuelcellstore.com.cob-web.org:8888 /cgi-bin/fuelweb/view=Item/cat=/product=52 (313 words)

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