Consider the following redox reaction with nitrogen (N): NO3 + H* + 8e +→ _NH4* a. Balance this redox reaction. b. What are the oxidation states of nitrogen in nitrate and ammonium? c. Is nitrate undergoing reduction or oxidation? d. Using the thermodynamic data in Appendix A of your textbook, calculate AGºrxn, log K, and EH° for the reaction.

12. Electrochemistry is important in many aspects of daily life. i. Define voltaic cell. ii. Fill in the blanks for the drawing of a voltaic cell that's made with copper/copper (II) nitrate (E° = 0.34 V) and zinc/zinc (II) nitrate (E° = -0.76 V). Briefly explain the role of the salt bridge. iii. Using the equation Eᵒcell = E° cathode E anode, calculate the overall cell potential for the cell in step b. Be sure to show all steps completed to arrive at the answer. h. a. b. C. d. e. 1845 f. g. h. b. C. 9- C. d. h

2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?

1.Ca metal is produced by electrolysis of __________. a.CaCl2 b.CaSO4 c.CaF2 d.CaCO3 2.Which hydroxide of group 1 metal is the LEAST soluble? a.KOH b.LiOH c.CsOH d.NaOH