iPad . 1:42 PM 95 % a session.masteringchemistry.com C) MasteringChemistry: Cour

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iPad . 1:42 PM 95 % a session.masteringchemistry.com C) MasteringChemistry: Course Home CH223 Winter 2015 MC11: Thermodynamics ± Cell Potential and Equilibrium Please Show Steps And Correct Answ MC11: Thermodynamics Signed in as Priscilla Pimentel Help Close Resources « previous evious 16 of 25 | next » The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation 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 Reduction half-reaction Eo (V) Ag+ (aq) + e-Ag(s) Cu2+ (aq) + 2e-Ca(s) Sn+(aq) 4e-Sn(s0.15 2H (aq) 2e-H2 (g) Ni2+ (aq) +2e-Ni(s) 0.26 Fe2+ (aq)+ 2e-Fe(s) | -0.45 Zn2+ (aq) + 2e-Zn(s) | -0.76 Al3+ (aq) +3e--Al(s) | -1.66 Mg2+ (aq) + 2e-Mg(s) | -2.37 0.80 0.34 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 (aq)-Fe2+ (aq) + Ni(s) Express your answer numerically. Submit Hints My Answers Give Up Review Part Part B Calculate the standard cell potential (E) for the reaction X(s) + Y+ (aq)X+ (aq) + Y(s) if K - 4.82x103 Express your answer to three significant figures and include the appropriate units. |B"= Value Units Submit Hints My Answers Give Up Review Part Provide Feedback Continue

Explanation / Answer

PART A

E0= 0.059/n *log Kc

E0Ni+2/Ni - E0Fe+2/Fe = 0.059/n *log Kc

-0.26+ 0.45 = 0.059/2 * logKc

Kc= 2.75 x106

PART B

E0= 0.059/n *log Kc

E0= 0.059/1 *log (4.82 x 10-3)

      = - 0.136 V

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