# 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 table**^{1}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 (Cu
^{2+}) to form Zn^{2+}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:

Cu^{2+}+ 2e^{-}$\, \rightleftharpoons \,$ Cu where E^{0}red = +0.34 V

Zn^{2+}+ 2e^{-}$\, \rightleftharpoons \,$ Zn where E^{0}red = -0.76 V

- During the reaction, the reaction quotient Q is measured to be 1.8*10
^{8}. 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 (Cu