WebThe known Faraday constant 96,485 C/mol denoted by the symbol F, or also called 1 F, corresponds to the amount of electricity that is carried by 1 mol of electrons. The number … WebMay 14, 2024 · asked May 14, 2024 in Chemistry by Ruksar (69.0k points) The standard Gibbs energy for the given cell reaction in kJ mol–1 at 298 K is : Zn (s) + Cu2+(aq) → Zn2+(aq) + Cu (s), Eº = 2V at 298 K (Faraday’s constant, F = 96000 C mol–1 ) (1) – 192 (2) 192 (3) – 384 (4) 384 jee mains 2024 Share It On 1 Answer +1 vote
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WebΔ G ° = − n F E cell ° Δ G ° = −2 × 96,485 C mol × 1.247 J C = −240.6 kJ mol The reaction is spontaneous, as indicated by a negative free energy change and a positive cell potential. The K value is very large, indicating the reaction proceeds to near completion to yield an equilibrium mixture containing mostly products. Check Your Learning WebThis amount of charge, equal to about 96 485 coulombs, became known as Faraday's constant. Later, it was adopted as a convenient unit for measuring the charges used in … song opportunities
Solved The standard free energy change for a reaction …
WebFeb 19, 2024 · The Faraday constant, F, is a physical constant equal to the total electric charge carried by one mole of electrons. The constant is named for English scientist Michael Faraday. The accepted value of the constant is: F = 96,485.3365 (21) C/mol F = 96 485.3329 s A / mol F = 23.061 kcal per volt gram equivalent F = 26.801 A·h/mol Weba) The standard free energy change for a reaction can be calculated using the equation. where n is the number of electrons transferred F is Faraday\'s constant, 96.5 … WebMar 31, 2024 · We know the relation between free energy change and cell potential is: ΔG₀ = - n F E⁰ where F = Faraday's constant = 96485 C/mol n = 2 (given by equation that the electrons involved is 2) ΔG₀ = - 2 x 96485 x E⁰ - 698 kJ = - 2 x 96485 x E⁰ E⁰ = (698 x 1000) / (2 x 96485) = 3.62 volts Advertisement Advertisement song ordinary world