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Cell Potentials at Standard Conditions

Cell Potentials at Standard Conditions. Revisiting E cell. Standard Reduction Potentials. Reduction potentials for many electrodes have been measured and tabulated. Standard Hydrogen Electrode. Their values are referenced to a s tandard h ydrogen e lectrode ( SHE ).

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Cell Potentials at Standard Conditions

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  1. Cell Potentials at Standard Conditions Revisiting Ecell

  2. Standard Reduction Potentials Reduction potentials for many electrodes have been measured and tabulated.

  3. Standard Hydrogen Electrode • Their values are referenced to a standard hydrogen electrode (SHE). • By definition, the reduction potential for hydrogen is 0 V: 2 H+(aq, 1M) + 2 e− H2(g, 1 atm)

  4.   Ecell = Ered (cathode) −Ered (anode) Standard Cell Potentials The cell potential at standard conditions can be found through this equation: Because cell potential is based on the potential energy per unit of charge, it is an intensive property.

  5.   Ecell Ered Ered = (anode) (cathode) − Sample Exercise 20.5 p.841 TREND ALERT! The more the , the greater the tendency for reduction under std conditions. Ered

  6. Oxidizing and Reducing Agents F2: Most + value, easily reduced, strongest oxidizing agent Li: Most – value, easily oxidized, strongest reducing agent

  7. Oxidizing and Reducing Agents p. 843 • The strongest oxidizers have the most positive reduction potentials. • The strongest reducers have the most negative reduction potentials.

  8. Oxidizing and Reducing Agents The greater the difference between the two, the greater the voltage of the cell.

  9. Sample Exercise 20.8 p. 845 WEAKEST …………………………………STRONGEST Ag+NO3-Cr2O7-2 NO3- = + 0.96 V Ag+ = +0.80 V Cr2O7-2 = +1.33 V

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