Looks up abbreviations and acronyms beginning with the letter E used in chemistry and chemical engineering.
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Well, the mathematical difference is E - E^@ = -(RT)/(nF)lnQ... The conceptual difference is nonstandard vs. standard conditions. We define standard conditions to be 25^@ "C" and "1 atm" pressure, with "1 M" concentrations. Many chemical functions, particularly in thermodynamics and electrochemistry, are temperature-dependent. Thus, we must be able to account for that... We recall that for the Gibbs' free energy: DeltaG = DeltaG^@ + RTlnQ (if you do not recall this equation, look here for a derivation.) and: DeltaG^@ = -nFE^@ (which I will not derive as it is a simple unit conversion.) The first equation uses RTlnQ as a correction factor for nonstandard conditions for the Gibbs' free energy. It turns out that the second equation also applies to the nonstandard DeltaG. Hence: -nFE = -nFE^@ + RTlnQ Dividing by -nF gives: bb(E = E^@ - (RT)/(nF)lnQ) which is the purest version of the Nernst equation (before any simplifications), where: n is the number of electrons transferred in the redox reaction F = "96485 C/mol e"^(-) is the Faraday constant. R and T are known from the ideal gas law. Q is the reaction quotient, i.e. not-yet-equilibrium constant. E is the "electromotive force" for the cell process. E^@ is, of course, E at standard conditions. Likewise, -(RT)/(nF)lnQ is a correction factor to "convert" from standard to nonstandard conditions. If we are at standard conditions, then... E = E^@ - cancel((("8.314472 J/mol"cdot"K")("298.15 K"))/(nF)ln(1))^(0) => E = E^@ at 25^@ "C", "1 atm" pressure, and "1 M" concentrations.
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Well, the mathematical difference is E - E^@ = -(RT)/(nF)lnQ... The conceptual difference is nonstandard vs. standard conditions. We define standard conditions to be 25^@ "C" and "1 atm" pressure, with "1 M" concentrations. Many chemical functions, particularly in thermodynamics and electrochemistry, are temperature-dependent. Thus, we must be able to account for that... We recall that for the Gibbs' free energy: DeltaG = DeltaG^@ + RTlnQ (if you do not recall this equation, look here for a derivation.) and: DeltaG^@ = -nFE^@ (which I will not derive as it is a simple unit conversion.) The first equation uses RTlnQ as a correction factor for nonstandard conditions for the Gibbs' free energy. It turns out that the second equation also applies to the nonstandard DeltaG. Hence: -nFE = -nFE^@ + RTlnQ Dividing by -nF gives: bb(E = E^@ - (RT)/(nF)lnQ) which is the purest version of the Nernst equation (before any simplifications), where: n is the number of electrons transferred in the redox reaction F = "96485 C/mol e"^(-) is the Faraday constant. R and T are known from the ideal gas law. Q is the reaction quotient, i.e. not-yet-equilibrium constant. E is the "electromotive force" for the cell process. E^@ is, of course, E at standard conditions. Likewise, -(RT)/(nF)lnQ is a correction factor to "convert" from standard to nonstandard conditions. If we are at standard conditions, then... E = E^@ - cancel((("8.314472 J/mol"cdot"K")("298.15 K"))/(nF)ln(1))^(0) => E = E^@ at 25^@ "C", "1 atm" pressure, and "1 M" concentrations.
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A coulomb (C) relates electrical potential, expressed in volts, and energy, expressed in joules. The faraday (F) is Avogadro’s number multiplied by the charge on an electron and corresponds to …
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Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element …
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Chemical Forums - Index
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This chemistry dictionary offers chemistry definitions commonly used in chemistry and chemical engineering starting with the letter E.
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Interactive 3D chemistry animations of reaction mechanisms and 3D models of chemical structures for students studying University courses and advanced school chemistry hosted by University of Liverpool
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You are watching: Top 13+ What Is E- In Chemistry
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