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Topic: Nernst equation

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Standard electrode potential

Electrochemical potential

Electrode potential

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Walther Hermann Nernst

Walther Nernst

Osmotic pressure

Electrochemical cell

Chemical potential

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	Highbeam Encyclopedia - Search Results for Nernst,
		The son of a Prussian judge, Nernst was educated at the universities of Zürich, Berlin...
		A Dictionary of Chemistry; 1/1/2004; 78 words; Nernst equation An equation that relates the electrode potential E of an electrode that is in contact with an ionic solution to...
		The equation was derived by Walther Nernst in 1889.
	www.encyclopedia.com /SearchResults.aspx?Q=Nernst, (1107 words)

	3. Subthreshold membrane phenomena
		Equation 3.21 is the famous Nernst equation derived by Walther Hermann Nernst in 1888 (Nernst, 1888).
		In Equation 3.34 the expression for sodium ion current is seen to be similar to that for potassium (except for exchanging Na for K); however, the expression for chloride requires, in addition, a change in sign in the exponential term, a reflection of the negative valence.
		The latter curve is the steady-state response and corresponds to Equation 3.49.
	butler.cc.tut.fi /~malmivuo/bem/bembook/03/03.htm (8503 words)

	Walther Nernst - Wikipedia, the free encyclopedia
		Nernst invented, in 1897, the Nernst lamp, an electric lamp using an incandescent ceramic rod (the successor to the carbon lamp and the precursor to the incandescent lamp).
		His Nernst glower, important in the field of infra-red spectroscopy, is a solid-body radiator with a filament of rare-earth oxides.
		Nernst died in 1941 and is buried near Max Planck in Göttingen, Germany.
	en.wikipedia.org /wiki/Walther_Nernst (472 words)

	Walther Hermann Nernst
		Nernst applied the principles of thermodynamics to the chemical reactions proceeding in a battery.
		He constructed an equation, known as the Nernst Equation, which related the voltage of a cell to its properties.
		Nernst and his students in Berlin proceeded to make many important physico-chemical measurements, particularly determinations of specific heats of solids at very low temperatures and of vapour densities at high temperatures.
	www.corrosion-doctors.org /Biographies/Nernst.htm (478 words)

	Nernst Equation
		Each ion has an equilibrium potential associated with it whereby the diffusive forces and the electrical forces balance.
		This is given by the Nernst Equation
		Generally people use the logarithm base 10 in which case the Nernst equation is multiplied by the factor 2.303.
	www.cnbc.cmu.edu /~bard/passive2/node2.html (96 words)

	Nernst equation - Wikipedia, the free encyclopedia
		In physiology the Nernst equation is used for finding the electric potential of a cell membrane with respect to one type of ion.
		The Nernst Equation may be derived in several different ways.
		The magnitude of the Nernst potential is determined by the ratio of the concentrations of that specific ion on the two sides of the membrane.
	en.wikipedia.org /wiki/Nernst_equation (973 words)

	Bloomfield Science Museum/Walther Hermann Nernst
		Nernst developed this theory, which is so important that it is called "The Third Law of Thermodynamics "and which had, and still has, great scientific and industrial importance.
		Of Nernst's many contributions to physical chemistry - the understanding of chemical principles in terms of underlying physical laws - one in particular is enshrined in the name "The Nernst Equation".
		It is the flow of these ions through pores in the membranes which form the walls of the tubes that sustains the passage of the electrical impulses, rather than the flow of electrons along wires as in technological communication devices such as telephones.
	www.mada.org.il /website/html/eng/2_1_1-18.htm (807 words)

	The Nernst Equation (Site not responding. Last check: 2007-10-26)
		Hermann Walther Nernst was born in Prussia in 1864.
		Nernst's first outstanding work was his theory of the electromotive force of the voltaic cell.
		Nernst is probably best known to electrochemists for his elucidation of the Nernst equation.
	www-biol.paisley.ac.uk /marco/enzyme_electrode/chapter2/nernst.htm (521 words)

	Sandwalk: Nobel Laureate: Walther Hermann Nernst
		Through the law of the conservation of energy, the first fundamental law of the theory of heat, it was possible on the one hand to calculate the change in the evolution of heat with the temperature.
		With the aid of his co-workers Nernst was able through extremely valuable experimental research to obtain a most remarkable result concerning the change in specific heats at low temperatures.
		In biochemistry he is responsible for the Nernst equation that relates standard reduction potentials and Gibbs free energy.
	sandwalk.blogspot.com /2007/05/nobel-laureate-walther-hermann-nernst.html (659 words)

	Sect. 1, Ch. 3: Goldman-Hodgkin-Katz Equation (Site not responding. Last check: 2007-10-26)
		Before this equation was developed, an equation based on the Nernst equation was used to predict the resting membrane potential of cells if both the permeability of all ions in solution and their concentrations on each side of the membrane were known.
		This equation is known as the Goldman-Hodgkin-Katz equation after the three physiologists who were responsible for its derivation.
		Because this equation is not in the form of a simple weighted average, it is cumbersome to use for predicting how the resting potential will respond to changes in permeability.
	www.lib.mcg.edu /edu/eshuphysio/program/section1/1ch3/s1ch3_24.htm (191 words)

	Walther Nernst Memorial
		The Nernst glower exhibits a bright emission in the visible spectrum (white light), and it was initially used for ordinary electric illumination.
		The Nernst lamp (patented 1897) could be operated in ambient air, whereas the carbon filament lamp of Thomas Edison (1879) required a vacuum environment which was quite a disadvantage.
		Stark, Johannes (1874 - 1957) Opponent of Nernst.
	www.nernst.de (1864 words)

	Princeton Applied Research - Fuel Cell
		The Nernst equation provides a relationship between the ideal standard potential (E°) for the cell reaction and the ideal equilibrium potential (E) at other temperatures and partial pressures of reactants and products.
		According to the Nernst equation for the hydrogen reaction, the ideal cell potential at a given temperature can be increased by operating at higher reactant pressures, and improvements in fuel cell performance have, in fact, been observed at higher pressures.
		Because CO is produced at the anode and consumed at the cathode in MCFCs, and because the concentrations in the anode and cathode feed streams are not necessarily equal, the CO partial pressures for both electrode reactions are present in the second Nernst equation shown in Table 2-2.
	www.princetonappliedresearch.com /products/markets/fuel_cell.cfm (1817 words)

	Nernst Equation (Site not responding. Last check: 2007-10-26)
		The voltage also depends on the concentration (for liquids) or pressure (for gaseous reactants) of the components in the redox reaction since the average energy of the components will be altered by changes in concentration or pressure.
		The voltage under conditions other than 1 M for solutions and 1 atm for gasses is given by the Nernst equation.
		A key implication of the Nernst equation is that the voltage of a battery is not necessarily constant, but varies as it is charged or discharged as the concentration of the components of the electrolyte changes.
	www.udel.edu /igert/pvcdrom/BATTERY/nernst.htm (304 words)

	Intute sciences - >Chemical Sciences: Electrochemistry: Introduction to the Nernst Equation
		The Nernst equation, in the form we shall use it, links the actual (measurable) reversible potential of an electrode, E, to the standard reversible potential of the electrode couple, E
		In general, it is more convenient to apply the Nernst equation to one electrode at a time, and we will do this.
		The Nernst equation will give the actual electrode potential no matter what form of the electrode reaction is used, as long as the form corresponds to a physically real couple.
	www.intute.ac.uk /sciences/reference/plambeck/chem2/p02101.htm (706 words)

	Nernst Equation
		His contribution to chemical thermodynamics led to the well known equation correlating chemical energy and the electric potential of a galvanic cell or battery.
		The Nernst equation also indicates that you can build a battery simply by using the same material for both cells, but by using different concentrations.
		0 = 1.100 - 0.0296 log ([Zn ] / [Cu The Nernst equation is useful for the determination of equilibrium constants.
	www.science.uwaterloo.ca /~cchieh/cact/c123/nernsteq.html (1234 words)

	Science in Poland - Walther Hermann Nernst
		Nernst had shown that it is possible to determine the equilibrium constant for a chemical reaction from thermal data, and in so doing he formulated what he himself called the third law of thermodynamics.
		But Nernst showed in 1906 that it is possible with the aid of the third law, to derive the necessary parameters from the temperature dependence of thermochemical quantities.
		To prove his heat theorem (the third law) Nernst carried out thermochemical measurements at very low temperatures, and such studies were extended in the 1920s by G.N. Lewis in Berkeley.
	www.staff.amu.edu.pl /~zbzw/ph/sci/whn.htm (537 words)

	THE NERNST PAGE
		Nernst knew that electrolytes existed both inside and outside of cells and he already had some idea of the concentrations of electrolytes in the major body water compartments, thanks to the work of our friend
		We might read the equation as negative 61 multiplied by the log of the concentration of an ion in the ICF, divided by the concentration of the same ion in the ECF.
		To tackle the equation, our first step is to enter the ion concentrations...
	faculty.etsu.edu /currie/study/nernst.htm (835 words)

	Developing Interactive Web Interfaces for Scientific and Medical Applications
		It may also be important for the equation to be run repeatedly with precise values.
		To see how the equation is laid out I will show it again with a light color for the hidden borders.
		Equations usually use a number of symbols that are not part of a normal keyboard.
	www.medicalcomputing.net /action_potentials_code.html (965 words)

	Standard Electrode Potentials
		The Nernst equation relates the cell potential to its standard cell potential.
		The quantity Q, the thermodynamic reaction constant, is like a dynamic version of the equilibrium constant in which the concentrations and gas pressures are the instantaneous values in the reaction mixture.
		The Nernst equation allows us to predict the cell potential for voltaic cells under conditions other than standard conditions of 1M, 1 atmosphere, 25°C. The effects of different temperatures and concentrations may be tracked in terms of the Gibbs free energy change
	hyperphysics.phy-astr.gsu.edu /hbase/chemical/electrode.html (1055 words)

	The Chemistry of Batteries (Site not responding. Last check: 2007-10-26)
		Walther H. Nernst received the Nobel Prize in 1920 for his contributions to the field of electrochemistry.
		This equation is known as the Nernst equation.
		It is also possible to conclude from the Nernst equation that it is possible to create a battery using the same material in the anode and the cathode but a different concentrations.
	www.uvm.edu /~swgordon/131-01/131web/sarasmoller/finalproject.html (2298 words)

	The Nernst/Goldman Equation Simulator
		The Nernst/Goldman Equation Simulator is provided "as is", without warranty of any kind.
		In no event shall the authors or copyright holders be liable for any claim, damages, or other liability out of or in connection with this software.
		Special thanks to the Arizona Board of Regents for funding the development of the Nernst/Goldman Equation Simulator.
	www.nernstgoldman.physiology.arizona.edu (339 words)

	Equilibrium Potentials
		For example it allows the measurement of pH using what is essentially a voltmeter measuring the equilibrium potential of protons between a reference solution on one side of a proton-permeable glass, and of an unknown concentration of protons in a test solution on the other side.
		But once we note that this description involves only the question of the concentration gradient and the electrical gradient for this one ion, we can see that the same relationship must apply for a membrane which might also be permeable to some other ions, provided the concentrations are not running down.
		through the opening of a population of ion selective channels), and that permeability were to be very large, the membrane potential that must result is that predicted by the Nernst equation for the concentration gradient that applied for the particular ion, for the the membrane is approximating a single ion selective one.
	www.physiol.usyd.edu.au /daved/teaching/nernst.html (887 words)

	Chemistry : Chapter 17 : Overview
		The minus in the equation changes the reduction potential to an oxidation potential, so a separate step is not necessary.
		To correct for nonstandard conditions, the Nernst equation is used to determine the cell potential (E
		Because the temperature effect is relatively small and most cells operate at room temperature, the cell potential in volts is often determined from a more convenient form of the Nernst equation, which assumes a temperature of 25 °C
	www2.wwnorton.com /college/chemistry/gilbert/overview/ch17.htm (986 words)

	Sandwalk: The Nernst Equation
		Just as the actual Gibbs free energy change for a reaction is related to the standard Gibbs free energy change by this equation, an observed difference in reduction potentials (ΔE) is related to the difference in the standard reduction potentials (ΔE°') by the Nernst equation.
		For a reaction involving the oxidation and reduction of two molecules, A and B, the Nernst equation is
		The Nernst equation is very famous but it's actually not very useful.
	sandwalk.blogspot.com /2007/05/nernst-equation.html (1355 words)

	The Net Equation: Your Online Source for Chemistry Solutions
		To cope with this discrepancy, Walter Nernst, a German chemist and physicist, developed an equation in the early 1900's to relate reduction potential, temperature, concentration, and moles of electrons transferred.
		This equation is quite powerful, because of its simplicity: the equilibrium constant can be determined for any redox reaction simply by knowing the standard reduction potential and the number of electrons transferred in the balanced equation.
		Using these three powerful equations, you can find the real cell potential at any concentration state and temperature, find the equilibrium constant, and find the Gibbs free energy value for use in thermodynamic calculations.
	library.thinkquest.org /C004970/redox/kdeltag.htm (351 words)

	Electrical Work and the Nernst Equation
		(The charge in Equation 12 is negative because electrons have a negative charge) The Faraday number is the number of coulombs of charge in one mole of (positive) electron charges.
		Equation 14 is the fundamental equation of electrochemistry because it relates the electromotive force (emf) of an electrochemical cell to the thermal properties of the chemical reaction carried out in that cell.
		In Equation 19 we have used Q not as charge but as a shorthand way to write the product and quotient of activities appearing in Equation 18.
	www.chem.arizona.edu /~salzmanr/480a/480ants/elecwork/elecwork.html (1094 words)

	chapter4
		If the Nernst equation is true, then the cell kinetics is log-form.
		Establishment of the Nernst equation from the electrochemical cell kinetics.
		The reconciliation of the Nernst equation with Langmuir kinetics is an example of the general
	www.geocities.com /astenzy/chapter4.html (1181 words)

	The Nernst/Goldman Equation Simulator
		Although absolute values for ionic permeability have been determined for selected cell types (under ‘selected conditions’), permeability ratios, that is, the relative permeability of a membrane to selected ions, are far more pertinent to understanding the impact of ion gradients on the electrical potential across a membrane.
		It’s also worth noting that When a membrane is permeable to only one species, the Nernst equation applies.
		However, when more than one ionic species can cross the membrane in response to prevailing electrochemical gradients, the GHK equation applies (within the limits imposed by the assumptions behind its derivation; see B. Hille, Ion Channels of Excitable Membranes, 3rd Ed., 2001), and the ratio of permeabilities is the relevant parameter.
	www.nernstgoldman.physiology.arizona.edu /using (1302 words)

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