Use the equipment above (See Attachment), as well as wires and a voltmeter, to construct a galvanic cell with the smallest possible value for E^o cell.
a. Write the balanced net ionic equation for the reaction that produces the smallest possible value for E^o cell.
b. Calculate the standard cell potential, E^o, in volts for the thermodynamically favored reaction that occurs in this cell.
c. Which metal is used at the anode, and which is used at the cathode?
d. What would be the voltage of this cell if it was constructed without a salt bridge? Explain.

Repeat All For largest possible value for E^o cell.

Ecell = E0cathode + E0 anode
Look at the reduction potential table to get minimum positive E0cell
You will fine that with Cu 2+ (reduction) at the cathode and Zn(s) oxidation on the anode
hence use Cu as cathode and Zn as anode .Without salt bridge ...no reaction hence no cell potential.
Repeat this for largest possible value for E0cell