Calculating cell potential (voltaic cells)

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Intros
Lessons
  1. Will a redox reaction occur?
  2. Reduction potential
  3. Will a redox reaction happen spontaneously?
  4. Will a redox reaction happen spontaneously? Worked example 1
  5. Will a redox reaction happen spontaneously? Worked example 2
  6. Cell potential, free energy and equilibrium.
  7. The Nernst equation (non-standard cell potential).
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Examples
Lessons
  1. Use a standard potential table1 to predict whether a spontaneous redox reaction will occur.
    1. Will a reaction between Cu (I) and nickel metal occur spontaneously in a redox process?
    2. Will a reaction between Al (III) and scandium metal occur spontaneously in a redox process?
    3. Will a reaction between vanadium metal and Scandium (III) occur spontaneously in a redox process?
  2. Calculate the equilibrium constant K using the cell potential and calculate the cell potential at nonstandard conditions.
    1. The oxidation of zinc metal (Zn) by copper ions (Cu2+) to form Zn2+ ions and Cu (s) happens spontaneously in a redox reaction at standard conditions at 298K. Calculate the equilibrium constant K for this process using the following standard potential data:

      Cu2+ + 2e- β€‰β‡Œβ€‰ \, \rightleftharpoons \, Cu where E0red = +0.34 V
      Zn2+ + 2e- β€‰β‡Œβ€‰ \, \rightleftharpoons \, Zn where E0red = -0.76 V
    2. During the reaction, the reaction quotient Q is measured to be 1.8*108. Use the Nernst equation to find the nonstandard cell potential at these conditions.
      Is the cell potential increasing, decreasing or unchanged during the reaction?