Consider the diagram and reaction below to select the best possible answer for the following questions . Ni (s) + 2Ag (aq) → Ni2+ (aq) + 2Ag (s) Object "X" Solid nickel Solution containing Ni²+ Cell A 1. Which cell is the cathode? [Select] 2. In which direction will the electrons flow? [Select] 3. What is the name of "Object X"? [Select] 4. What is the purpose of "Object X" [Select] Cell B Solid silver Solution containing Ag¹+

5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.

How many moles of Al3+ would be electrolyzed to Al(s) with the same amount of electricity that produces 16.0 g Cu(s) from a solution of Cu(NO3)2?

A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.

> A Moving to the next question prevents changes to this answer. uestion 28 The half-reaction occurring at the anode in the balanced reaction shown below is 3MNO 4 (aq) + 24H * (aq) + 5Fe (s) → 3Mn 2+ 3+ (aq) + 5Fe (aq) + 12H 20 (O O Fe (s) → Fe2+ (aq) + 2e O 2MN04 (aq) + 12H (aq) + 6e 2MN2+ (aq) + 3H20 (1) Fe2+ (aq) – Fe3+ (aq) + e Fe (5) → Fe3+ (aq) + 3e" O Mn04 (aq) + 8H* (aq) + 5e → Mn2+ (aq) + 4H20 (1) A Moving to the next question prevents changes to this answer. 93 OType here to search

Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)