CH302 LaBrake and Vanden Bout Electrochemical Cells Experimental Observations of Electrochemical Cells 1. Consider the voltaic cell that contains standard Co 2+ /Co and Au 3+ /Au electrodes. The following experimental observations were noted: (1) Metallic gold plates out on one electrode and the gold ion concentration decreases around that electrode, and (2) The mass of the cobalt electrode decreases and the cobalt (II) ion concentration increases around that electrode. a. Diagram this voltaic cell. Make sure to b. Diagram the cell using the short hand notation <Co(s) Co 2+ (aq) Au 3+ (aq) Au(s)> c. What is the standard cell potential of this voltaic cell? E cell = E cathode - E anode = 1.50 V (- 0.28 V) = 1.78 V 2. Consider the electrolysis of molten calcium chloride with inert electrodes. The following experimental observations were noted: (1) Bubbles of pale green chlorine gas are produced at one electrode, and (2) Silvery white molten metallic calcium is produced at the other electrode.
a. Diagram this electrolytic cell. Make sure to b. Diagram the cell using the short hand notation <Pt(s) Cl - (aq) Cl2(g) Ca 2+ (aq) Ca(s) Pt(s)>, you can use any kind of inert electrodes, here we used platinum c. What is the standard cell potential of this electrolytic cell? E cell = E cathode - E anode = - 2.76 V (1.36 V) = - 4.12 V 3. Problem 1 is an example of a galvanic or voltaic cell. Problem 2 is an example of an electrolytic cell. Considering the diagrams of these two cells, what are the differences and similarities between galvanic (voltaic) cells and electrolytic cells? Differences between the galvanic and electrolytic cells are the galvanic cell has a positive standard cell potential while the electrolytic cell has a negative one, the signs of the cathode and anode are reversed, and there is a battery in the electrolytic cell and not in the galvanic cell.
Similarities are oxidation happens at the anode and reduction happens at the cathode in both, anions go towards the anode and cations go towards the cathode in both, electrons flow towards the cathode and the current goes towards the anode in both, and the standard cell potential is calculated using the same equation. Short Hand Notation of Electrochemical Cells 4. Consider the following cell <Ni(s) Ni 2+ (aq) Ag + (aq) Ag(s)> a. Diagram this cell. Make sure to b. What is the standard cell potential of this cell? E cell = E cathode - E anode = 0.80 V (- 0.23 V) = 1.03 V c. Is this cell a galvanic cell or an electrolytic cell? Galvanic, because E cell is positive 5. NEW PROBLEM: Consider the following cell <Pt(s) Ce 3+ (aq) Ce 4+ (aq) Cu 2+ (aq) Cu(s)>
a. Diagram this cell. Make sure to b. What is the standard cell potential of this cell? E cell = E cathode - E anode = 0.34 V (1.70 V) = - 1.36 V c. Is this cell a galvanic cell or an electrolytic cell? Electrolytic, because E cell is negative
Electrochemical Cell Diagrams 6. Consider the following cell: a. Would you assume this cell is a voltaic or an electrolytic cell? Why do you think this? We would assume this cell is an electrolytic cell because it includes a battery or power source. b. Knowing this complete the diagram of this cell by i. Indicating the anode, cathode, positive and negative electrodes ii. Writing out the ½ reactions and their type occurring at each electrode iii. Writing out the overall balanced redox reaction that goes with this cell iv. Labeling the direction of electron flow and the current v. Labeling the direction of anions and cations in the salt bridge
c. What is the short hand notation for this cell? <Cu(s) Cu 2+ (aq) Zn 2+ (aq) Zn(s)> d. What is the standard cell potential of this cell? E cell = E cathode - E anode = - 0.76 V (0.34 V) = - 1.10 V 7. Consider the following cell: a. Would you assume this cell is a voltaic or an electrolytic cell? Why do you think this? We would assume this cell is a galvanic cell because it does not include a battery or power source and is powering a light bulb. b. Knowing this complete the diagram of this cell by i. Indicating the anode, cathode, positive and negative electrodes ii. Writing out the ½ reactions and their type occurring at each electrode iii. Writing out the overall balanced redox reaction that goes with this cell iv. Labeling the direction of electron flow and the current v. Labeling the direction of anions and cations in the salt bridge
c. What is the short hand notation for this cell? <Zn(s) Zn 2+ (aq) Cu 2+ (aq) Cu(s)> d. What is the standard cell potential of this cell? E cell = E cathode - E anode = 0.34 V (- 0.76 V) = 1.10 V 8. The cells in problems 6 and 7 have almost the same components. However, one is galvanic and one is electrolytic. What are some of the similarities and differences between these two problems? Differences between the galvanic and electrolytic cells are the galvanic cell (problem 7) has a positive standard cell potential while the electrolytic cell (problem 6) has a negative one, the signs of the cathode and anode are reversed, and there is a battery in the electrolytic cell and not in the galvanic cell. Similarities are oxidation happens at the anode and reduction happens at the cathode in both, anions go towards the anode and cations go towards the cathode in both, electrons flow towards the cathode and the current goes towards the anode in both, and the standard cell potential is calculated using the same equation.