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Table of Standard Reduction Potentials in Aqueous Solution This table tells you the electrical energy given off by the reduction reaction, under standard conditions (25oC, 1 M concentrations of everything). Negative values means energy has to be put in to drive the reduction reaction. High values of E0 means the chemical species is very easily reduced. An oxidation reaction is the reverse of a reduction reaction. Flipping the reaction also flips the sign of the energy. So oxidation reaction towards the bottom of the table occur more easily than those towards the top. For instance reduction of Cl2 to chloride ions gives off a lot of energy because chlorine loves electrons. Oxidation of Cl– ions back to Cl2 would instead require a lot of energy. C re l2(g) + easily O 2(g) + duced Cathode (Reduction) Half-Reaction Standard Potential E° (volts) 2.01 1.36 1.23 0.90 0.59 0.52 0.35 0.34 0.22 0.17 0.16 0.00 -0.83 -2.38 -2.71 loves electrons S2O82-(aq) + 2e- -> 2SO42-(aq) eq) 2 4 ClO-(aq) C C C H e- -> 2H2O(l) (l) + 2e- -> Cl-(aq) + 2OH-(aq) O(l) + 2e- -> ClO-(aq) + 2OH-(aq) Cu(s) lO2-(aq) + H2 u+(aq) + e- -> lO3-(aq) + H2 u2+(aq) + 2e- - gCl(s) + e- -> lO4-(aq) + H2 - -> har +(oaxqi) + H2O 2Cl-(a d to di+ze4 O(l) + 2e- -> ClO2-(aq) + 2OH-(aq) > Cu(s) C A C C 2 2H2O(l) + 2e- -> H2(g) + 2OH-(aq) Mg2+(aq) + 2e- -> Mg(s) Ag(s) + Cl-(aq) O(l) + 2e- -> ClO3-(aq) + 2OH-(aq) u2+(aq) + e- -> H+(aq) + 2e- - Cu+(aq) > H2(g) hard to reduce easily oxidized hates electrons Na+(aq) + e- -> Na(s) Created by LABScI at Stanford 11PDF Image | Electrolysis splitting water
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