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The equilibrium constant, K. for a redox reaction is related to the standard cell potential, E by the equation cell nFE In K cel RT where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 98 500 C mol. R (the gas constant) is equal to 8.314 JKmol and Tis the Kelvin temperature.

The equilibrium constant, K. for a redox reaction is related to the standard cell potential, E by the equation cell nFE In K cel RT where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 98 500 C mol. R (the gas constant) is equal to 8.314 JKmol and Tis the Kelvin temperature.

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The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E. by the equation Standard reduction potentials In K = nFE Reduction half-reaction E (V) RT Ag+(ag) +eAg(s) 0.80 where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 98 500 C mol-1, R(the gas constant) is equal to 8.314 JK-' mol1. and T is the Kelvin temperature. Cu2+ (ag) + 20 Cu(s) 0.34 Sn+(ag) + 4e-Sn(s) 0.15 2H+(ag) + 20H2(9) Ni+ (ag) + 2e-»Ni(s) Fe+ (ag) + 20Fe(s) Zn2+ (ag) + 2e→Zn(s) -0.26 -0.45 -0.76 A1+ (ag) + 30-Al(s) -1.68 Mg+ (ag) + 20MB(s) 2.37 • Part A Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + N+ (ag) »Fe2+ (ag) + Ni(s) Express your answer numerically. > View Available Hint(s) ? K =
Transcribed Image Text:The equilibrium constant, K, for a redox reaction is related to the standard cell potential, E. by the equation Standard reduction potentials In K = nFE Reduction half-reaction E (V) RT Ag+(ag) +eAg(s) 0.80 where n is the number of moles of electrons transferred, F (the Faraday's constant) is equal to 98 500 C mol-1, R(the gas constant) is equal to 8.314 JK-' mol1. and T is the Kelvin temperature. Cu2+ (ag) + 20 Cu(s) 0.34 Sn+(ag) + 4e-Sn(s) 0.15 2H+(ag) + 20H2(9) Ni+ (ag) + 2e-»Ni(s) Fe+ (ag) + 20Fe(s) Zn2+ (ag) + 2e→Zn(s) -0.26 -0.45 -0.76 A1+ (ag) + 30-Al(s) -1.68 Mg+ (ag) + 20MB(s) 2.37 • Part A Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + N+ (ag) »Fe2+ (ag) + Ni(s) Express your answer numerically. > View Available Hint(s) ? K =
Part B Calculate the standard cell potential (E cel for the reaction X(s) +Y*(ag) X+(ag) + Y(s) if 6.51 x 10 . Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit
Transcribed Image Text:Part B Calculate the standard cell potential (E cel for the reaction X(s) +Y*(ag) X+(ag) + Y(s) if 6.51 x 10 . Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? Value Units Submit
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