For the reaction between metallic iron (Fe (s)) and cupric
sulfate (CuSO4 (aq)) that produces ferrous sulfate (FeSO4 (aq)) and
copper (Cu (s)) that occurs in a voltaic cell:
a) Write the reaction
b) What is the reducing agent?
c) What is the oxidizing agent?
d) Write the oxidation half reaction
e) Write the reduction half-reaction
f) Calculate the standard potential of the cell
g) Is the reaction spontaneous? justify your answer
For The Reaction Between Metallic Iron Fe S And Cupric Sulfate Cuso4 Aq That Produces Ferrous Sulfate Feso4 Aq 1 (93.21 KiB) Viewed 48 times
19.1 Standard Reduction Potentials at 25°C ° Half-Reaction MnO2 (aq) + 2H2O + 3e → Mnoz(s) + 40H(aq) 12(s) + 2e-21-(aq) O2(g) + 2H20 + 4e -40H(aq) Cu²+ (aq) + 2e" - Cu(s) AgCl(s) + e-Ag(s) + Cl (aq) so (aq) + 4H+ (aq) + 2e - SO,(g) + 2H2O Cu2+ (aq) + e- Cu (aq) Snº+(aq) + 2e ) + Sn? (aq) + 2H+(aq) + 2e - H2(g) → Pb2+ (aq) + 2e - Pb(s) Sn2+ (aq) + 2e Sn(s) Ni2+ (aq) + 2e Ni(s) Co2+ (aq) + 2e Co(s) PbSO4(s) + 2e Pb(s) + 5O2 (aq) Cd2+ (aq) + 2e Cd(s) Fe2+ (aq) + 2e -> Fe(s) Cr3+ (aq) + 3e" - Cr(s) Zn²+(aq) + 2e - Zn(s) 2H2O + 2e-H2(g) + 2OH(aq) E°(V) +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83
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