The cell diagram of a mercury cell can be written
Zn(s) | ZnO (s) NaOH (aq) HgO (s) HgO (I)
(a) Write the electrode reactions and cell reaction with electron number z = 2.
(b) Use data in Appendix H to calculate the standard molar reaction quantities ΔrH°, ΔrG°, and ΔrS° for the cell reaction at 298.15K.
(c) Calculate the standard cell potential of the mercury cell at 298.15K to the nearest 0.01V.
(d) Evaluate the ratio of heat to advancement, ξq / dξ, at a constant temperature of 298.15K and a constant pressure of 1 bar, for the cell reaction taking place in two different ways: reversibly in the cell, and spontaneously in a reaction vessel that is not part of an electrical circuit.
(e) Evaluate dE°cell,eq= dT , the temperature coefficient of the standard cell potential.