1. The problem statement, all variables and given/known data 2. Consider an electrochemical cell as shown, with Zn in ZnCl2(aq) and Cu in Cu(NO3)2(aq), and a salt bridge containing KNO3(aq). The overall chemical reaction is Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s). a. How many moles of electrons are transferred in this reaction? b. Which side is the anode?. c. Which direction will electrons travel? d. Which material is being reduced? e. What is the oxidizing agent? 2. Relevant equations a for a i understand that 2 moles of electrons are transferred throught the salt brige. From anode to cathode.for b i said that the left side is the anode and c) that the electrons travel from zinc to copper for d: o recognize that Cu 2+ is being reduced because it gains 2 electrons and becomes Cu (s). for e i think that since Cu 3+ is rduced it is the oxidizing agent.. 3. The attempt at a solution but my professor says the electrons flow from copper to zinc andthat zinc is the oxidizing agent...can anyone explain?