1. Solve for the following electrochemical cell:

Positive electrode: Pb²⁺ + 2e- Pb

Negative electrode: PbSO₄ + 2e- Pb + SO₄^2-

(a) Determine the electrode potentials at standard conditions and calculate corresponding cell voltage. Assume that the standard electrode potential is shown by the table below

(b) What is the dependence of cell voltage on the concentration of Pb²⁺ and SO₄^2- in the solution?

(c) If the activities of pure solids are 1, and the solubility product is defined as [Pb²⁺][SO₄^2-]. Calculate the solubility product.

(d) Recalculate the solubility product at 80 degrees C, and if the voltage of the cell has a temperature coefficient of -1 mV/K.

Table of standard electrode potentials Legend: (s) - solid; (l) - liquid; (g) - gas; (aq) - aqueous (default for all charged species); (Hg) - amalgam; bold - water electrolysis equations