Calculating cell potential (voltaic cells)
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Intros
Lessons
- Will a redox reaction occur?
- Reduction potential
- Will a redox reaction happen spontaneously?
- Will a redox reaction happen spontaneously? Worked example 1
- Will a redox reaction happen spontaneously? Worked example 2
- Cell potential, free energy and equilibrium.
- The Nernst equation (non-standard cell potential).
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Examples
Lessons
- Use a standard potential table1 to predict whether a spontaneous redox reaction will occur.
- Calculate the equilibrium constant K using the cell potential and calculate the cell potential at nonstandard conditions.
- 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- Cu where E0red = +0.34 V
Zn2+ + 2e- Zn where E0red = -0.76 V
- 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?
- 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: