Use the given half reactions to "construct" an electrolytic cell. Zn^2+ + 2 e^>Zn E°cell = -0.76 V Cu^2+ + 2 e^> Cu E°cell = 0.34 V 1. Predict the standard potential of the cell at 298 K. 2. What is the minimum voltage that should be applied to the standard electrolytic cell found in question to cause zn2+ to be reduced to Zn?

See explanation and image attached

Explanation:

The standard cell potential at 298 K is given by;

E°cathode - E°anode

Hence;

E°cell = 0.34 V - (-0.76 V)

E°cell = 0.34 V + 0.76 V

E°cell = 1.1 V

To reduce Zn^2+ to Zn then Zn must be the cathode, hence;

E°cell = (-0.76 V) - 0.34 V

E°cell = -1.1 V

explanation:

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