1. Draw a picture of the lab apparatus and include:
1a. The cathode is the electrode (terminal) at which reduction occurs. Write the correct half cell reaction (at bottom of side of U tube that you say it occur) including number of electron moving
1b. The other electrode, the anode, is where oxidiation occurs. Write the correct half cell reaction (at bottom of side of U tube that you say it occur) including number of electron moving
1c. Indicated on the drawing the type of material you used for each electrode (you symbol of the electrode can look a "t" with a long body and no hook at bottom.
1d. Alligator clips and wire (called Leads) can be shown as lines and battery can be a box with the word "Battery" or capital letter P (also could put the actual symbol for battery).
2. Underneath the picture, write the complete/molecular chemical reaction. Then show all work in determining what is oxidized, what is reduced, what is oxidizing agent, what is reducing agent and balance the Redox by Oxidation Number.
3a. Leave some blank space and then write each half cell and put the voltage for each half cell (you determine from Standard Reduction Potential Table given to you) to the far right side of the line you wrote the half cell reaction on. Stack two lines of information as if you were adding them (which you are going to do!). Then put an addition line below it and then add the two half cell together to the overall balanced chemical reaction. Add the voltages of the two half cells to get the Ecell for the overall reaction (also called cell).