Problem: Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq) Cl2(g) + 2e- → 2 Cl-(aq)                      E° = +1.36 VFe3+(aq) + 3e- → Fe(s)                       E° = -0.04 VA) +4.16 VB) -1.40 VC) -1.32 VD) +1.32 VE) +1.40 V

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cell    =    cathode   —   anode
               (reduction)     (oxidation)

Usually:

• Larger E°cell = cathode
• Smaller E°cell = anode

BUT if an equation or a reaction is given:

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Problem Details

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)

3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq)

Cl2(g) + 2e- → 2 Cl-(aq)                      E° = +1.36 V
Fe3+(aq) + 3e- → Fe(s)                       E° = -0.04 V

A) +4.16 V

B) -1.40 V

C) -1.32 V

D) +1.32 V

E) +1.40 V

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