Nernst equation

Nernst e·qua·tion

(nārnst),

the equation relating the equilibrium potential of electrodes to ion concentrations; the equation relating the electrical potential and concentration gradient of an ion across a permeable membrane at equilibrium: E = [RT / nF] [ln (C₁/C ₂)], where E = potential, R = absolute gas constant, T = absolute temperature, n = valence, F = the Faraday, ln = the natural logarithm, and C₁ and C₂ are the ion concentrations on the two sides; in nonideal solutions, concentration should be replaced by activity.
See also: activity (2).

Farlex Partner Medical Dictionary © Farlex 2012

Nernst e·qua·tion

(nernst ĕ-kwā'zhŭn)

The equation relating the equilibrium potential of electrodes to ion concentrations; the equation relating the electrical potential and concentration gradient of an ion across a permeable membrane at equilibrium: E = [RT/nF] [ln (C₁/C₂)], where E = potential, R = absolute gas constant, T = absolute temperature, n = valence, F = the Faraday, ln = the natural logarithm, and C₁ and C₂ are the ion concentrations on the two sides; in nonideal solutions, concentration should be replaced by activity.
See also: activity (2)

Medical Dictionary for the Health Professions and Nursing © Farlex 2012

Nernst,

Walther, German physicist and Nobel laureate, 1864-1941.

Nernst equation - the equation relating the electrical potential and concentration gradient of an ion across a permeable membrane at equilibrium.

Nernst potential

Nernst theory - that the passage of an electric current through tissues causes a dissociation of the ions.

Medical Eponyms © Farlex 2012

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References in periodicals archive ?

He is famous for developing the Nernst Equation in 1887.

In electrochemistry, the Nernst equation is an equation that relates the reduction potential of an electrochemical reaction (half-cell or full cell reaction) to the standard electrode potential, temperature, and activities (often approximated by concentrations) of the chemical species undergoing reduction and oxidation.

Corrosion - Occurrence and Prevention

The linear relationship between the concentration ratio of [I.sub.2]/KI solution and the ORP value was obtained through Nernst equation. [I.sub.2]/KI electrode solutions with concentration ratios of 1:4 (0.1 M [I.sub.2] and 0.4 M KI), 1:8 (0.1 M [I.sub.2] and 0.8 M KI), 1:12 (0.1 M [I.sub.2] and 1.2 M KI), 1:16 (0.1 M [I.sub.2] and 1.6 M KI), and 1:20 (0.1 M [I.sub.2] and 2 M KI) were used to verify the linear relationship.

Establishment of a Method for Measuring Antioxidant Capacity in Urine, Based on Oxidation Reduction Potential and Redox Couple [I.sub.2]/KI

[21] has applied the Nernst equation, mass balance equation of redox reaction and Faraday's law of electrolysis to establish the relationship between the half-cell redox concentration of Ce(IV)/Ce(III) and the ORP during electrolysis.

Estimating the state-of-charge of all-vanadium redox flow battery using a divided, open-circuit potentiometric cell

Nernst equation for the above reaction can be written as follows,

Ethanol extract of Musa acuminate peel as an eco-friendly inhibitor for the corrosion of mild steel in [H.sub.2]S[O.sub.4]

The half-cell potential for each reaction is determined with the Nernst equation. The resulting corrosion rate is dependent upon temperature and species concentrations at the metal-solution interface.

Modelling carbon dioxide corrosion with film crystallization and erosion

Josowicz, 'A Fresh Look at Some Old Principles, The Kelvin Probe and the Nernst Equation', Anal.

Challenges and Opportunities of Modern Electrochemistry

See Appendix D for the derivation of the Nernst Equation. Table II The equilibrium potential (in V) of each ion across the plasma membrane and vacuolar membrane of a characean internodal cell and the plasma membrane of a squid nerve.

The excitability of plant cells: with a special emphasis on Characean internodal cells

Figure 2 shows the potential-pH diagram is drawn using the Nernst equation. The figure shows that it is possible to synthesize cobalt particles using hydrazine because the oxidation potential of hydrazine is less noble than the reduction potential of cobalt.

Synthesis and characterization of cobalt nanoparticles using hydrazine and citric acid

The measurement reaction is based on Nernst equation:

Monitoring system with broad band wireless data collection

Electrochemistry: Oxidation/reduction; anode/cathode; galvanic/electrolytic cells; half reactions; Nernst equation; electrolysis; chloralkali process; Hg, Ni/Cd, Pb batteries; electroplating.

Development of a first-year chemistry course with emphasis on environmental chemistry

(Note that the energies are the Gibbs energy changes for the balanced half reactions, referred to the element as arbitrary zero, and not the Gibbs energies of formation of the ions.) They are easily calculated from redox couples and where necessary the solubility products of the hydroxides using the Nernst equation and the familiar relationship: