An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode

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?

A cell is constructed by immersing a strip of silver in 0.10 M AgNO 3 solution and a strip of lead in 1.0 M Pb(NO 3) 2 solution. A wire and salt bridge complete the cell. What is the potential of the silver electrode in the cell? O a. 0.80 V O b. 0.83 V O C. 0.88 V O d. 0.86 V e. 0.74 V

22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)