Chapter 18, Lecture 2

Chapter 18, Lecture 2 - CH 18 Lecture 2 Page 1 CH 18...

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CH 18 Lecture 2 Page 1
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CH 18 Lecture 2 Page 2 STANDARD ELECTRODE POTENTIALS All referenced to the STANDARD HYDROGEN ELECTRODE Eº H + / H 2 = 0.000 V TABLE 18.1 STANDARD ELECTRODE POTENTIALS AT 25 ºC Acidic Solution Volts F 2 (g) + 2 e - 2 F - + 2.866 S 2 O 8 -2 (aq) + 2 e - 2 SO 4 -2 (aq) + 2.01 MnO 4 - (aq) + 8 H + + 2 e - Mn +2 (aq) + 4 H 2 O (l) + 1.51 PbO 2(s) + 4 H + + 2 e - Pb + (aq) + 2 H 2 O (l) + 0.1.455 Fe +3 (aq) + e - Fe +2 (aq) + 0.771 2 H + (aq) + e - H 2 (g) 0.000 Pb +2 + 2 e - Pb (s) - 0.125 Zn +2 (aq) + 2 e - Zn (s) - 0.763 Li + (aq) + e - Li (s) - 3.040 Basic Solution OCl - (aq) + H 2 O (l) Cl - (aq) + 2 OH - + 0.890 2 H 2 O (l) + 2 e - H 2 (g) + 2 OH - - 0.828 THE BEST OXIDIZING AGENTS, THOSE MOST EASILY REDUCED, APPEAR HIGH IN THE TABLE.
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CH 18 Lecture 2 Page 3 WE CAN EASILY DETERMINE THE STANDARD POTENTIAL, Eº cell , OF A CELL FROM THE DATA IN THE TABLE. Zn (s) Zn +2 Cu +2 (aq) Cu (s) cell = Eº (anode) - Eº (cathode) E º cell = Eº Cu + (aq) \ Cu (s) - Eº Zn (s) / Zn + (aq)
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Chapter 18, Lecture 2 - CH 18 Lecture 2 Page 1 CH 18...

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