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Topic: Table of standard electrode potentials

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	Standard Electrode Potentials
		This potential is a measure of the energy per unit charge which is available from the oxidation/reduction reactions to drive the reaction.
		The electrode potential depends upon the concentrations of the substances, the temperature, and the pressure in the case of a gas electrode.
		The standard electrode potentials are customarily determined at solute concentrations of 1 Molar, gas pressures of 1 atmosphere, and a standard temperature which is usually 25°C. The standard cell potential is denoted by a degree sign as a superscript.
	hyperphysics.phy-astr.gsu.edu /hbase/chemical/electrode.html (1055 words)

	UNIT 8* - ADDITIONAL MATERIALS IN REDOX AND ELECTROCHEMISTRY (Site not responding. Last check: 2007-11-03)
		To obtain the equation and the potential for the oxidation half-reaction, the equation as written in the table must be reversed, and the sign of E° changed.
		Therefore, to obtain the equation and the potential for this oxidation half-reaction, the equation for magnesium as written in the table must be reversed and the sign of E° changed.
		NOTE: The Standard Electrode Potentials (E°) are not multiplied by the coefficients in calculating the E° for the reaction.
	dwb.unl.edu /Chemistry/LearningObjectives/NY08x.html (875 words)

	Standard electrode potential - Wikipedia, the free encyclopedia
		This potential difference is created as a result of the difference between individual potentials of the two metal electrodes with respect to the electrolyte.
		Since the oxidation potential of a half-reaction is the negative of the reduction potential in a redox reaction, it is sufficient to calculate either one of the potentials.
		is the standard potential at the cathode as given in the table of standard electrode potential.
	en.wikipedia.org /wiki/Electrode_potential (740 words)

	unit04-sect02-les02-lessona (Site not responding. Last check: 2007-11-03)
		The electrical potential (E) or cell potential of the electrochemical cell is a function of the half-cell combination.
		The Standard Reduction Potentials of Half-Cells Table was constructed by building electrochemical cells using the standard hydrogen electrode and measuring cell potentials.
		Look-up the standard reduction potentials of the anode and cathode.
	www.cdli.ca /courses/chem3202/unit04/section02/lesson02/3-lesson-a.htm (1310 words)

	Reference Electrodes (Site not responding. Last check: 2007-11-03)
		The electrode is a silver wire that is coated with a thin layer of silver chloride either by electroplating or by dipping the wire in molten silver chloride.
		The potential of the electrode remains constant as long as the chloride concentration remains constant.
		The reference electrode is immersed into an intermediate volume filled with an electrolyte solution that is connected to the main chamber of the cell with a Luggin capillary.
	chem.ch.huji.ac.il /~eugeniik/refelectrodes.htm (2100 words)

	redox reactions (Site not responding. Last check: 2007-11-03)
		You should be able to link the electrodes with the reduction and oxidation taking place in the electrode compartment, and predict the direction of the flow of electrons in an external circuit.
		Standard electrode potentials: You should understand the principle of cell electromotive force as the difference in the standard electrode potentials of two half-cells, and the meaning of the term standard electrode potential.
		You should be able to use a table of standard electrode potentials in order to calculate the e.m.f.
	web.uct.ac.za /depts/emu/cbe/REDOX.HTM (183 words)

	Chem1 Electrochemistry: cell potentials and thermodynamics
		In particular, if we adopt a reference half-cell whose potential is arbitrarily defined as zero, and measure the potentials of various other electrode systems against this reference cell, we are in effect measuring the half-cell potentials on a scale that is relative to the potential of the reference cell.
		Standard [reduction] potentials are commonly denoted by the symbol E°.
		A table of standard half-cell potentials summarizes a large amount of chemistry, for it expresses the relative powers of various substances to donate and accept electrons by listing reduction half-reactions in order of increasing E° values, and thus of increasing spontaneity.
	www.chem1.com /acad/webtext/elchem/ec3.html (3271 words)

	CHEM 111 Summer 2003 Study Guide (Site not responding. Last check: 2007-11-03)
		Be able to calculate the standard Gibbs free energy of reaction from tables of standard enthalpies of formation and standard entropies.
		Know that the electrode potential of the standard hydrogen electrode is defined as 0.000 V. Be able to use the table of standard electrode potentials to predict the spontaneous direction of a redox reaction.
		Be able to use the table of standard electrode potentials to calculate the standard cell potential of an electrochemical cell.
	www.towson.edu /~debye/chem111/2003s/111_03s_st.html (2106 words)

	The Nernst Equation (Site not responding. Last check: 2007-11-03)
		The Table of Standard Reduction Potentials and the Nernst Equation
		First we shall define the "cell potential" in terms of the anode and cathode potentials, and determine the amount of work that can be extracted from a voltaic cell.
		The individual electrode potentials will then be associated with the tendency of the electrode half-reaction to occur.
	www.owlnet.rice.edu /~chem122/lecture/Outlines/lect19.html (94 words)

	Physical Chemistry Oxidation- Reduction
		Relative electrode potentials are determine by comparison with a standard hydrogen electrode which is assigned a value of zero under standard thermodynamic conditions.
		The potential difference between the standard hydrogen electrode and other redox couples in which the concentration of the active ions in solution is effectively molar at at temperature of 298 K is known as the standard electode potential (or redox) potential.....
		In the table below the half reaction is the state of equilibrium in which the reduced element is in equilibrium with the oxidised state (the element ions).
	www.roymech.co.uk /Related/Chemistry/Chem_Oxidation.html (637 words)

	Standard Electrode Potentials
		After studying this section, you will (a) know the meaning of the term "standard electrode potential", (b) understand the relationship between the electromotive force of a cell and the standard electrode potentials of its half cells, (c) be able to use a table of standard electrode potentials in order to calculate the e.m.f.
		The cell potential (emf) of this cell under standard conditions is 1.10 V (volt).
		The emf of the cell (1.10 V) is the potential difference between the electrodes of the cell, which is the difference between the abilities of the half-cells to attract electrons.
	www.physchem.co.za /Redox/SEP.htm (650 words)

	Corrosion
		Which metal will undergo oxidation is determined by the ‘standard electrode potential’, which is measured against an arbitrary zero created by a ‘standard hydrogen electrode’.
		Table 2 gives standard electrode potentials for many of the metals used in electronic packaging – the more positive the electrode potential, the more ‘noble’ the metal is, and hence the less prone to oxidise and hence corrode.
		Corrosion can occur with no external applied potential, and is merely dependent on the thermodynamic free energy of the reaction – if that free energy is negative (that is, heat is given out) then the reaction will take place spontaneously.
	www.ami.ac.uk /courses/topics/0157_corr (925 words)

	NM WAIDS Corrosion Theory
		These standard potentials are measured with respect to the standard hydrogen electrode (SHE).
		To determine oxidation potentials, reverse the direction of the arrow and reverse the sign of the standard potential.
		Table 1 can be used to show that copper will corrode in nitric acid solutions (oxidizing) and aerated water.
	octane.nmt.edu /waterquality/corrosion/theory.htm (1177 words)

	Table of standard electrode potentials - KnowledgeIsFun.com (Site not responding. Last check: 2007-11-03)
		The standard electrode potentials are used to determine the electrochemical potential or the electrode potential of an electrochemical cell or Galvanic cell.
		These electrode potentials are experimentally calculated with the standard hydrogen electrode, because one cannot determine the voltage from the chemical equations.
		The values below are standard electrode potentials taken at 298 K, 1 bar pressure and in aqueous solution, of concentration 1 molar.
	www.knowledgeisfun.com /T/Ta/Table-of-standard-electrode-potentials.php (214 words)

	Section 6.5.2
		The resulting potential, read directly in millivolts from a potentiometer (such as a pH meter), is corrected for the difference between the standard potential of the reference electrode being used at the solution temperature and the potential of the standard hydrogen electrode
		E° = 430 mV is the standard electrode potential of ZoBell's solution measured against the hydrogen electrode at 25°C. Half-cell potentials for the calomel, silver:silver chloride, and combination electrodes are shown in table 6.5-2.
		table 6.5-3, the equipment is ready for field use.
	water.usgs.gov /owq/FieldManual/Chapter6/6.5.2.html (714 words)

	Failure due to humidity
		The severity of electromigration increases with applied potential gradient, the time to grow dendrites decreasing both with reducing electrode spacing and increasing voltage.
		The levels given in Table 3 are related to specific test conditions which are applied before reflow soldering and evaluation.
		Standard conditions start at 85ºC/85% relative humidity (RH), but more severe tests are frequently specified, in order to test the limits of the latest encapsulating processes.
	www.ami.ac.uk /courses/topics/0125_fdh/index.html (3001 words)

	UNIT 4 - PERIODIC TABLE (Site not responding. Last check: 2007-11-03)
		The atomic number is the basis of the arrangement in the present form of the periodic table.
		The normal covalent radius is the effective distance from the center of the nucleus to the outer valence shell of that atom in a typical covalent or coordinate bond.
		The ionization energy decreases with increasing atomic number because of the increased distance of the valence electron(s) from the nucleus and also because of the increased shielding effect produced as new occupied energy levels are added to the atom.
	dwb.unl.edu /Chemistry/LearningObjectives/NY04.html (2326 words)

	Foundations of Electronics - Standard Potentials (Site not responding. Last check: 2007-11-03)
		Examples of using the standard reduction potential table are given.
		The potentials are constant, even if the amount of each molecule is increased or decreased, provided the ratios remain the same.
		We find the potentials for these reactions is the table of standard reduction potentials.
	library.thinkquest.org /10784/chem5.html (319 words)

	17
		The property that is most used for this purpose is the standard potential of the electrode at which the half reaction occurs in an electrochemical cell, Eº.
		This can be used to work out the direction in which a complete reaction will tend to go, since the more positive the value of Eº, the stronger the tendency for the half reaction to proceed in the direction of taking up electrons.
		From a table of standard electrode potentials given in a textbook, predict the direction of the following reaction
	www.hull.ac.uk /chemistry/intro_inorganic/Chap17-2.htm (470 words)

	Chemistry 30 Electrochemistry - Standard Electrode Potentials
		This force is known as the potential difference or electromotive force (emf or E).
		Potential difference is measured in volts (V), and thus is also referred to as the voltage of the cell.
		Tables of Standard Reduction Potentials for Half-Reactions allow us to determine the voltage of electrochemical cells.
	www.saskschools.ca /~chem30_dev/6_redox/redox2_3.htm (571 words)

	studyq_electrochem.html
		Given that the standard cell voltage is 0.35 V, and that the standard reduction potential of chlorine is 1.36 V:
		Determine the standard emf of a cell that uses Ag/Ag and Al/Al half-cell reactions.
		A voltaic cell consists of a hydrogen electrode and a Cu/Cu2+ electrode.
	lamar.colostate.edu /~kw2/c113/studyq_electrochem.html (437 words)

	[No title]
		Examine a table of standard electrode reduction potentials and determine whether the following statements are true or false.
		From the cell potential calculate the value of the equilibrium constant for the reaction at 25(C. From the equilibrium constant, or the reaction, calculate the standard free energy change for the reaction.
		Using an applied potential of 5.0V to overcome kinetic effects, and a current of quarter million amps, a.
	www.chemmybear.com /groves/apch21_studyqxn.doc (589 words)

	Conquering Chemistry HSC Module 1
		The superscript o means that the value of the physical quantity – in this case the electrode potential – is the value at the standard state: this means that gases are present at exactly one atmosphere and solutes at an activity (effective concentration) of exactly one mole per litre.
		This corresponds to the listing of electrode potentials in order of increasing values (–2.9 and –2.7 V for K and Na to +1.2 and +1.7 V for Pt and Au), so as the electrode potential increases the reducing strength of the reduced form of the redox couple decreases (Ag is a weaker reductant than Zn).
		Another way of summarising reactivity in terms of the table of electrode potentials is to say that the half reaction with the higher electrode potential has the greater tendency to occur.
	www.cci.net.au /conqchem/HSCmod1text.htm (5165 words)

	CHEM 111.001 Spring 2001 Study Guide (Site not responding. Last check: 2007-11-03)
		Be able to write the autoionization reaction for water and know the values of the hydroxide ion and hydronium ion concentrations in pure water.
		Be able to calculate the standard Gibbs free energy of reaction from tables of standard heats of formation and standard entropies.
		Know that electric potentials and potential differences are measured in volts (V); that electric charge is measured in coulombs (C).
	www.towson.edu /~debye/chem111/S2002/111_s02st.html (2157 words)

	Learn more about List of reference tables in the online encyclopedia. (Site not responding. Last check: 2007-11-03)
		You usually find a collection of reference tables in the back of almanacs, dictionaries and encyclopedias (or an index of them, if they're scattered throughout the work).
		List of standards topics (these could easily be cross-referenced under other relevant categories as well)
		TLAs: Table of all possible TLAs from AAA to DZZ, to HZZ, to LZZ, to PZZ, to TZZ, to XZZ, to ZZZ
	www.onlineencyclopedia.org /l/li/list_of_reference_tables.html (1071 words)

	BCH 4053 Biochemistry I (Site not responding. Last check: 2007-11-03)
		The standard reduction potential for a reduction reaction involving any compound is determined by coupling to the hydrogen reaction and measuring the voltage of such a cell.
		A positive value for the standard reduction potential means that a compound in question preferentially is reduced when involved in a redox reaction with hydrogen.
		The information in the table of standard reduction potentials can be used to solve for the energy change associated with a particular redox reaction.
	wine1.sb.fsu.edu /BCH4053/Lecture38/Lecture38.htm (2801 words)

	[No title]
		You should be familiar with the relation between cell emf and the change in Gibbs free energy for the net cell reaction and be able to calculate equilibrium constants from standard electrode potentials.
		You should be able to use the Nernst equation to calculate electrode potentials under other than standard conditions (including the emf of a concentration cell).
		You should review the material in Chapter 4 on oxidation-reduction reactions (Section 4) and understand the relation between standard electrode potentials and the activity series presented there.
	www.utm.edu /departments/cens/chemistry/Old_Site/Chap20.htm (229 words)

	Chemistry Home
		The tables are currently being presented in GIF format.
		A table of Physical Constants including name, symbol, value and units for a variety of useful constants.
		A table of standard units, metric prefixes, conversion factors, and symbols.
	www.caton.org /chem1.php (413 words)

	Course Syllabus - CHEM1412
		Draw a potential energy versus reaction pathway diagram that illustrates the effect of a catalyst.
		Use standard free energies of formation to calculate the standard free energy change for a chemical process.
		Using a table of standard electrode potentials calculate the standard cell potential of a voltaic cell.
	www.tc.cc.tx.us /syllabus/?course=CHEM1412 (2031 words)

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