The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE°

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: The Equilibrium Constant K For A Redox Reaction Is Related To The Standard Potential Eo By The Equation In K Nfe 1 (35.81 KiB) Viewed 87 times

: The Equilibrium Constant K For A Redox Reaction Is Related To The Standard Potential Eo By The Equation In K Nfe 2 (51.09 KiB) Viewed 87 times

: The Equilibrium Constant K For A Redox Reaction Is Related To The Standard Potential Eo By The Equation In K Nfe 3 (37.29 KiB) Viewed 87 times

The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol. K), and T is the Kelvin temperature.

Standard reduction potentials E° (V) 4+ Reduction half-reaction Ag+ (aq) +eAg(s) 0.80 Cu2+ (aq) + 2e →Cu(s) 0.34 Snº+ (aq) + 4e +Sn(s) 0.15 2H+ (aq) + 2e →H2(g) 0 Ni2+ (aq) + 2e →Ni(s) -0.26 Fe2+ (aq) + 2e →Fe(s) -0.45 Zn²+ (aq) + 2e --Zn(s) -0.76 A13+ (aq) + 3e-Al(s) -1.66 Mg2+ (aq) + 2e- Mg(s) -2.37

Part B Calculate the standard cell potential (Eº) for the reaction X(s) +Y+ (aq)-X+ (aq) +Y(s) it K = 1.13x10-3 Express your answer to three significant figures and include the appropriate units. View Available Hint(s) μΑ ? E = Value V Submit Previous Answers * Incorrect; Try Again: 5 attempts remaining