a) Using standard reduction potentials, identify the anode and the cathode and determine the cell potential for a galvanic cell composed of copper and iron. Assume standard conditions.

Question

a) Using standard reduction potentials, identify the anode and the cathode and determine the cell potential for a galvanic cell composed of copper and iron. Assume standard conditions.

b) Confirm that the potential of the following galvanic cell is 0.462 V:

Answer 1

Cu²⁺ + 2e- ==> Cu(s) ... E^o = 0.34 V

Fe²⁺ + 2e- ==> Ag(s) ... E^o = -0.41 V

Since 0.34 is greater than -0.41, reduction will be the Cu reaction and oxidation will be the Fe reaction.

a) Anode = Cu and cathode is Fe

E^o = 0.34 + 0.41 = 0.75 V

b) Cu²⁺ + 2e- ==> Cu(s) E^o = 0.34 V

Ag⁺ + e- ==> Ag(s) E^o = 0.80 V

E^o = 0.80 - 0.34 = 0.46 V (your standard reduction potentials may vary slightly from the ones I used)