Standard Reduction Potentials at 25°C E° (volts) F2(g) + 2e →2F-(aq) +2.87 Au3+ + 3e → Au(s) +1.50 Cl2(g) + 2e → 2Cl(aq)

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Standard Reduction Potentials At 25 C E Volts F2 G 2e 2f Aq 2 87 Au3 3e Au S 1 50 Cl2 G 2e 2cl Aq 1 (47.6 KiB) Viewed 58 times

Standard Reduction Potentials at 25°C E° (volts) F2(g) + 2e →2F-(aq) +2.87 Au3+ + 3e → Au(s) +1.50 Cl2(g) + 2e → 2Cl(aq) +1.36 O2(g) + 4H30+(aq) + 4e + 6H2O(1) +1.23 Br2(1) + 2e → 2Br(aq) +1.08 Agt(aq) + → Ag(s) +0.80 Hg22+(aq) + 2e → 2Hg(1) +0.79 12(s) + 2e → 21:(aq) +0.535 Cu2+(aq) + 2e → Cu(s) +0.337 Sn++(aq) + 2e → Sn2+(aq) +0.15 Sn2+(aq) + 2e → Sn(s) -0.14 Cd2+(aq) + 2e → Cd(s) -0.40 Zn2+(aq) + 2e → Zn(s) -0.763 2H2O(l) + 2e → H2(g) + 2OH-(aq) -0.828 A13+(aq) + 3e + Al(s) -1.66 K+(aq) + → K(s) -2.93 Li*(aq) +eLi(s) -3.045 6. Using data from the reduction potential table and the reaction 2Ag(s) + Pt2+(aq) → Pt(s) + 2Ag+(aq) E°=0.38 V ( calculate the standard reduction potential of the half-reaction Pt2+(aq) + 2e → Pt(s) a) -1.18 V d) 1.18 V b) -0.40 V e) 2.00 V c) 0.40 V 7. Using data from the reduction potential table, predict which of the following is the best oxidizing agent? a) F2 d) Agt b) Ag e) A13+ c) Sn4+