The reaction in the Daniell cell is Cu2+ + Zn → Cu + Zn2+. (a) Given the following standard electrode potentials: Eo298K (Zn | Zn2+) = − 0.763 V; Eo298K (Cu | Cu2+) = + 0.337 V, calculate ΔGo for the cell reaction at 298 K. [−212.3] (b) If for the temperature coefficient of the cell potential, (?Eo / ?T)P is −1.08 x 10−4 V K−1, calculate ΔSo and ΔHo for the cell reaction at 298 K. [−212.3; −20.8; −218.5] The answers are in the bracket, I would like to know how they were obtained. Thank you!

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A: a.

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A: given data are-  Fe(s) ⟶ Fe2+(aq) + 2e-Eo = -0.44 V  O2(g) + 4H+(aq) + 4e- ⟶  2H2O(l)  Eo = 1.23 V…

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Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.