The equilibrium constant, K for a redox reaction is related to the standard pote

Question

The equilibrium constant, K for a redox reaction is related to the standard potential. E^o, by the equation ln K = nFE^o/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. Use the table of standard potentials given above to calculate the equilibrium constant at standard temperature (25 degree C) for the following reaction: Fe(s) + Ni^2+ (aq) rightarrow Fe^2+ (aq) + Ni(s) Express your answer numerically. K = Calculate the standard cell potential (E^o) for the reaction X(s)+Y^+(aq) rightarrow X^+(aq) + Y(s) if K =8.34 times 10^3. Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

Fe (s) + Ni+2 (aq) -----> Fe+2 (aq) + Ni (s)
E0 cell = E0 cathode - E0 anode
E0 cell = -0.26 -(-0.45)
E0 cell = 0.19
lnK = nFE0 cell / RT
lnK = 2 * 96500 * 0.19 / (8.314 * 298)
K = 2.678 * 10^6

given K = 8.34 * 10^-3
lnK = nFE0 cell / RT
ln(8.34 * 10^-3) = 1 * 96500 * E /(8.314 * 298)
E0 cell = -0.1229 v

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