+ Cell Potential and EquilibriumThe equilibrium constant, K, for a redox reaction is related to the standardpotential, E, by the equationIn K FERTwhere 72 is the number of moles of electrons transferred, F (the Faradayconstant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to8.314 J/(mol K), and T is the Kelvin temperature.Standard reduction potentials▾ Part AUse the tableExpress your answer numerically.▸ View Available Hint(s)K=ΥΠΙ ΑΣΦ 9Reduction half-reactionAg+ (aq) +eAg(s)Cu²+ (aq) +201>Cu(s)Sn+ (aq) + 4e →→Sn(s)2H+ (aq) +2e →H₂(g)Ni2+ (aq) + 2e →Ni(s)Fe²+ (aq) + 2e →Fe(s)Zn²+ (aq) +2e →Zn(s)Al³+ (aq) + 3e →Al(s)Mg²+ (aq) + 2e →Mg(s)standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction:Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s)?E (V)0.800.340.1500.26-0.450.76-1.662.3729 oReview | Constants | Period Part BCalculate the standard cell potential (E) for the reactionif K = 8.82x10-³Express your answer to three significant figures and include the appropriate units.▸ View Available Hint(s)SubmitValueUnitsX(s) +Y+ (aq) X+ (aq) +Y(s)?

Answered: Image /qna-images/answer/f533e901-6886-4e33-9c0b-ff2c9d372427.jpg

+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 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 ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) 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) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period

+ Cell Potential and Equilibrium The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation nFE RT In K where 11 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 ▼ Part A Express your answer numerically. View Available Hint(s) K= IVE ΑΣΦ ] + Reduction half-reaction Ag (aq) +eAg(s) Cu²+ (aq) + 2e Sn (aq) + 4e Sn(s) 2H+ (aq) +2e →>H₂(g) ? Ni²+ (aq) + 2e Fe2+ (aq) +2e Zn²+ (aq) + 2e AP (aq) + 3e Mg2+ (aq) + 2e Cu(s) 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) + Ni²+ (aq) >Fe²+ (aq) + Ni(s) E° (V) 0.80 0.34 0.15 0 -0.20 Ni(s) 0.45 Fe(s) Zn(s) Al(s) Mg(s) -2.37 0.76 -1.68 < 29 o Review Constants | Period

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Cu = reduction potential of +0.52. Mg is in pic. Thanks
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