ONLY #1 Metals in Aqueous Solutions by electrowinning

ONLY #1 from the sheet attached. These questions are like chemistry. I need help with these problems involving material engineering and chemistry to see how metals are reduced from oxides. These rxns are like batteries where electrons flow from one area to another. This is a quiz that I already did, but I left something out because I only got partial credit. So could you please help me by showing your work for the solution, so that I may see what I did wrong. Remember ONLY #1 from the sheet attached. Thanks for your time.

galvanic cells and faraday's laws

1. Diagram the following galvanic cell (or just tell what it would look like), indicating the direction of flow of electrons in the external circuit and the motion of ions in the salt bridge. Ni(s)lNi2+(aq)llHCl(aq)lH2(g)lPt(s). Also write a balanced equation for the overall reaction in this cell. 2. In the Hall-Heroult for the electrolytic production of aluminum, Al3+ ions from Al2O3 dissolved in molten cryolite (Na3AlF6) are reduced to Al(l) while carbon is oxidized to CO2 by reaction with oxide ions. (a)Write balanced equations for the half reactions at the anode and at the cathode and for the overall cell reaction. (b)If a current of 50,000 A is passed through the cell for a perio... click for more

Electrolyte concentration and polarization potential

ONLY #5. Hello, could you solve question #5 showing most of your work. I'd like to use it as a study guide. 5*. a) A copper refining cell is operating with an electrolyte which contains 0.05 m Sn2+. At what concentration of Cu2+ will the tin start to plate out in preference to the copper? The cell temperature is 40°C. b) A polarization potential arises from a concentration difference between ions in the neighborhood of the electrode and those in the bulk of the electrolyte solution. Calculate the polarization potential in a copper electrorefining cell given the following information. Cell temperature: 40°C Cu2+ concentration in the bulk of the solution: 1.0 m Cu2+ c... click for more

electrolysis of aqueous solutions

A .100 M neutral aqueous CaCl2 solution is electrolyzed using platinum electodes. A current of 1.50 A passes through the solution for 50.0 hours. (a) Write the half-reactions occuring at the anode and at the cathode (b) What is the decomposition potential? (c) Calculate the mass, in grams, of the product formed at the cathode.

kinetics question

the problem is attached. Note that M is a neighboring molecule. It could be an N2O5 molecule or an inert gas molecule.