Reference no: EM132925790

Activity - Electrolytic Cells

Question 1: Go to the Experiment section of the computer simulation. Use the computer simulation to set-up a Cu-Cu electrochemical electrolysis cell and to help you diagram the components of your cell.

a. Which copper metal electrode is the more active metal? Explain how you decided.

b. Write the net ionic equation for the cell reaction. Calculate E°cell . Is this reaction spontaneous?

c. Write the half-reaction occurring at the copper electrode connected to the negative end of the battery.

d. Write the half-reaction occurring at the copper electrode connected to the positive end of the battery.

e. Indicate on the diagram i.) the cathode, ii.) the anode, iii.) the direction of electron flow in this cell, iv) what hops on or hops off at each electrode (click-on the magnifying glass symbol while your simulation is running), v.) which electrode gains mass, which loses mass.

f. Calculate the mass of copper deposited when 8.00 Amps are forced into the cathode for 15.0 minutes.

Question 2: A metal electrode and a copper spoon are placed in 1.00 M aqueous zinc nitrate solution. The electrodes are connected to a battery capable of passing a current of 8.00 amperes. The goal is to plate zinc metal on the copper spoon. Go to the Experiment section of the Electrolysis Computer Simulation and set up an electrolysis cell designed to deposit zinc metal onto copper. Use the computer simulation to help you diagram the components of your cell (above) and to help answer the following questions.

a. Write the chemical reaction representing copper metal reacting with 1.00 M zinc nitrate to produce zinc metal and copper(II) nitrate. Calculate E°cell for this reaction. Is this reaction spontaneous or nonspontaneous?

b. Write the half-reaction that must occur at the spoon electrode in order to plate zinc metal on the spoon.

c. In-order to plate zinc metal onto the copper spoon, which terminal of the battery (positive or negative end) will you connect the spoon? Indicate this on the diagram. Explain.

d. In-order to plate zinc onto the copper spoon, the other electrode should be what type of metal? Which terminal of the battery (positive or negative end) will you connect this electrode? Put this information on your diagram. Write the half-reaction occurring at this metal electrode.

e. Run your computer simulation and use it to diagram your electrolysis cell. Indicate on the diagram above i.) the cathode, ii.) the anode, iii.) the direction of electron flow in this cell, iv) what hops on or hops off at each electrode (click-on the magnifying glass symbol)? v.) which electrode gains mass, which loses mass?

f. Calculate the mass of zinc deposited when 8.00 Amps are forced into the cathode for 15.0 minutes. Compare this mass to the mass of copper deposited on the copper electrode you calculated in 1f.

g. Compare the moles of zinc deposited on the spoon to the moles of copper deposited on the copper electrode in 1f. Comment. If you electrolyzed aluminum using 8.0 Amps for 15.0 minutes would the moles change?

Attachment:- Electrolytic Cells.rar