Using the following standard reduction potentials Fe³⁺(aq) + e^- → Fe²⁺(aq) E° = +0.77 V
Pb²⁺(aq) + 2 e^- → Pb(s) E° = -0.13 V
Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions.
Pb²⁺(aq) + 2 Fe²⁺(aq) → 2 Fe³⁺(aq) + Pb(s)

Question

Quizplus · Accepted Answer

To calculate the standard cell potential, we need to add the two half-cell reactions together in the correct orientation and cancel out any species that appear on both sides of the equation. First, we reverse the second half-cell reaction to match the overall reaction. PbS1U1P12 + S1S1P0(aq) + 2 e- <-> Pb(s) E° = +0.13 V Next, we add the two half-cell reactions. FeS1U1P13 + S1S1P0(aq) + Pb(s) <-> 2 FeS1U1P12 + S1S1P0(aq) + PbS1U1P12 The cell potential E° is the sum of the reduction potentials of the half-cell reactions. E° = E°(cathode) - E°(anode) = +0.13 V - (+0.77 V) = -0.64 V Since the standard cell potential is negative, the reaction is nonspontaneous under standard conditions.

Using the Following Standard Reduction Potentials Fe3+(aq)+ E- → Fe2+(aq)E°

Using the Following Standard Reduction Potentials Fe³⁺(aq)+ E^- → Fe²⁺(aq)E°