- From A Table Of Standard Reduction Potentials Fe2 Aq 2e Fe S E 0 447 V A13 Aq 3 E Al S E 1 662 V A 1 (22.8 KiB) Viewed 29 times
From a table of Standard Reduction Potentials: Fe2+ (aq) + 2e → Fe(s) E=-0.447 V A13+ (aq) + 3 e- + Al(s) E=-1.662 V a)
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From a table of Standard Reduction Potentials: Fe2+ (aq) + 2e → Fe(s) E=-0.447 V A13+ (aq) + 3 e- + Al(s) E=-1.662 V a)
From a table of Standard Reduction Potentials: Fe2+ (aq) + 2e → Fe(s) E=-0.447 V A13+ (aq) + 3 e- + Al(s) E=-1.662 V a) Which species gets oxidized? b) What is the overall balanced reaction? c) Calculate the cell potential E at 25°C for the reaction. d) What is the cell potential at non-standard conditions given that [Fe2+] = 0.020 M, [A13+] = 0.10 M.
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