2020年3月6日 · Re: Units G=-nFE Post by Nathan Nakaguchi 1G » Fri Mar 06, 2020 11:15 pm Volts = Joules/Coulomb so in deltaG=-nFE the Coulombs cancel out from the multiplication between E (J/C) and F (C/mol), and n has no units so the final units will be J/mol.

2016年3月28日 · I was reviewing one of my missed destroyer questions (#158 in the 2015 Destroyer), and it was to calculate ∆G. From what I understand, n is the number of moles of electrons. The problem gave the reduction and oxidation reaction: one had 3 electrons transferred, the other had 2 electrons transferred.

2020年3月9日 · Re: G=-nFe Post by 405268063 » Mon Mar 09, 2020 6:45 am Yes, you basically just need to know that however many electrons you have in your overall balanced equation will be plugged into n.

2020年2月26日 · Re: delta G = -nFE Post by Jasmine W 1K » Mon Mar 02, 2020 12:58 am The negative is to make sure that when E is positive, delta G will be negative, meaning that the reaction would be spontaneous.

2019年2月24日 · Re: Finding n in Delta G = -nFE Post by Andrew Bennecke » Mon Feb 25, 2019 6:16 am This is the value of moles of electrons that cancel in each of the half reactions before writing the whole net ionic equation.

2020年3月1日 · In the equation delta G = -nFEcell, the n = mol e-, F = 96485 J/V.mol e-, and Ecell = V. When these variables are multiplied, the mol e- and V cancel out, leaving just the J.

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2015年2月4日 · That's the general form of the Nernst equation. Note that n here refers to the number of moles of electrons that move around in the reaction (e.g. if LiCl to Li+ + Cl- is a one-electron process - you take an electron from Li and put it on Cl). What you wrote is the equilibrium Nernst equation. At equilibrium, delta G = 0. Thus, E = 0 by delta G ...

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