The standard cell potential (E°_cell)for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when [Zn²⁺] = 3.5 M and [Pb²⁺] = 2.0 × 10^-4 M. Pb²⁺ (aq)+ Zn (s)→ Zn²⁺ (aq)+ Pb (s) A)0.50 B)0.84 C)0.39 D)0.76 E)0.63

Question

Quizplus · Accepted Answer

The Nernst equation is used to calculate the cell potential under non-standard conditions: E = E° - (RT/nF) * ln(Q). Here, E° = 0.63 V, n = 2, and Q = [Zn²⁺]/[Pb²⁺] = 3.5/(2.0 × 10⁻⁴). Plugging in these values and using R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol, the calculated E is approximately 0.50 V.

The Standard Cell Potential (E°cell)for the Reaction Below Is +0

The Standard Cell Potential (E°_cell)for the Reaction Below Is +0