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Cell potentials and Reduction potentials

This guide explores the fundamental concepts of cell potentials and reduction potentials in electrochemistry. It covers key principles, including how voltages can be increased by arranging cells in series and the significance of the standard reduction potentials. The content further explains how to identify which half-cell gains electrons and determines reduction potential values, alongside the calculation of electrochemical cell voltages. Ideal for chemistry students, this resource simplifies complex ideas into readable segments.

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Cell potentials and Reduction potentials

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  1. Cell potentials and Reduction potentials

  2. Answers 1 - 5 1. The difference is “ ° ” - indicating 25°C and 1 M concentrations (1) 2. Voltages can be increased by arranging cells in series (1) (or changing concentrations) 3. “A measure of the tendency of a given half-reaction to occur as a reduction” (1) 4. The half-cell with the greater reduction potential will gain electrons (1) 5. The Cu half-cell has the greater reduction potential (1), since it is gaining electrons (1) /6

  3. Answers 6 - 10 6. The Fe half-cell has the greater reduction potential (1) 7. E°cell = E°reduced - E°oxidized (1) (E°cell = standard reduction potential of substance reduced - standard reduction potential of substance oxidized) 8. 0.62 V (1) 9. There is no way to measure the standard reduction potential of an isolated half-cell (1) A reference/standard electrode is chosen (1) 10. Cu has the greatest reduction potential (1) /6

  4. Answers 11 - 14 11. 0.00 V is the reduction potential for the hydrogen electrode (1) 0.00 V is arbitrarily set; it’s 0 by definition (1) 12. It has a lower reduction potential than the hydrogen electrode (1) 13. Either oxidation OR reduction can occur depending upon what the half-cell is coupled with (1) 14. E°cell = E°reduced - E°oxidized E°cell = E°Fe2+ – E°Mg2+ 1.96 V = -0.41 V – E°Mg2+ (1) E°Mg2+ = -0.41 V – 1.96 V = -2.37 V /5

  5. Answers 15 - 18 15. 5.92 V (1) by a F2 - Li cell (1) 16. a) 1.42 V - -0.25 V = 1.67 V (1) b) 0.80 V - 0.34 V = 0.46 V (1) c) -1.66 V - -2.37 V = 0.71 V (1) d) 0.34 - - 0.44 V = 0.78 V or 0.77 V - 0.34 V = 0.43 V (1) 17. Yes (1) because the larger reduction potential will be reduced, the smaller will be oxidized (E°cell = E°reduced - E°oxidized) 18. Yes (1) because you are subtracting a smaller (or more negative) number from a larger number /8, /25 For more lessons, visit www.chalkbored.com

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