A zinc half-cell is made with 1.00×10−3MZn(NO3)3 solution and a zinc electrode. A nickel half-cell is made with 1.00×10−3MNi(C2H3O2)2 solution and a nickel electrode. (a) To make a spontaneous voltaic cell, which half-cell needs to undergo oxidation and which half-cell will undergo reduction? Explain why. (b) If you were to set up the voltaic cell mentioned in Question 4a, how would you construct your cell? Please indicate which electrode the (+) or red lead is connected to and what direction are the electrons supposed to flow. (c) Describe what is happening at each electrode when the cell is complete. i. Anode: ii. Cathode: (d) If the cell bridge is filled with a concentrated KNO3 solution, to which half-cell will K+flow from the salt bridge. Briefly explain. (e) Write out the net ionic reaction for this voltaic cell. Don't forget stoichiometry! (f) Predict the voltage generated by this voltaic cell? (g) Will you observe the same voltage if the concentration of Ni(C2H3O2)2 solution is changed to 1.00×10−4M while the concentration of Zn(NO3)2 solution is still 1.00×10−3M. Explain why.