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.) 2 Ag⁺(aq) + Pb(s) → 2Ag(s) + Pb²⁺(aq)
Ag⁺(aq) + e- → Ag(s) E°= 0.80 V
Pb²⁺(aq) + 2 e- → Pb(s) E°= -0.13 V

Question

Quizplus · Accepted Answer

The standard cell potential can be calculated using the formula: E°cell = E°reduction (cathode) - E°oxidation (anode) In this case, the reduction occurs at the cathode where Ag^and are reduced to Ag, and oxidation occurs at the anode where Pb is oxidized to Pb^{2 and}. Therefore, E°cell = E°reduction (Ag⁺ → Ag) - E°oxidation (Pb → Pb²⁺) E°cell = 0.80 V - (-0.13 V) E°cell = 0.93 V The answer is choice A.

Use the Standard Half-Cell Potentials Listed Below to Calculate the Standard