g What is the standard cell potential for the following reaction occurring in an electrochemical cell. The equation is balanced. 3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq) The following data may be helpful: Cl2(g) + 2 e- → 2 Cl-(aq) Eº = 1.36 V Fe3+(aq) + 3 e- → Fe(s) Eº = -0.036 V a) -1.40 V b) 1.40 V c) 2.84 V

b) 1.40 V

Explanation:

Oxidation half equation;

2Fe(s) → 2Fe3+(aq) + 6 e-

Reduction half equation;

3Cl2(g) + 6 e- → 6 Cl-(aq)

E°cathode= 1.36 V

E°anode= -0.036 V

E°cell= E°cathode - E°anode

E°cell= 1.36 -(-0.036)

E°cell= 1.36 + 0.036

E°cell= 1.396 V

E°cell= 1.40 V

c. 75.7

i think that is the right

b) nuclear ive learned that in a pedtrodic table