1. A galvanic (voltaic) cell consists of an electrode composed of magnesium in a 1.0 M magnesium ion solution and another electrode composed of copper in a 1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. 

2.The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.43-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3 (aq). The Sb3 (aq) is completely oxidized by 30.4 mL of a 0.120 M aqueous solution of KBrO3(aq). The unbalanced equation for the reaction is:
BrO3^-(aq) + Sb^3+(aq)---> Br^-(aq)+Sb^5+(aq) 
Calculate the amount of antimony in the sample adn its percentage in ore.

3.A current of 3.87 A is passed through a Cr(NO3)2 solution for 1.10 hours. How much chromium is plated out of the solution? in (g)

4.A current of 4.85 A is passed through a Cu(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 7.60 g of copper?

5. Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00 M solutions of their ions. a) If connected as voltaic cells in series, which two metals are plated, and what is the total potential? b) If connected such that one cell acts as a battery to power the other as an electrolytic cell, which two metals are plated, and what is the total potential? c) If 3.00 g of metal is plated in the voltaic cell, how much metal is plated in the electrolytic cell? in (g).

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