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13 Dec 2019

3. If you had an endless supply of potatoes from which to make a battery, is there a maximum voltage that can be achieved? Phrased another way, what are the half reactions when you make a one cell battery? What are the half reactions when you have two cells, three cells, 1000 cells, and so on… Explain your reasoning.

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Nelly Stracke
Nelly StrackeLv2
16 Dec 2019

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Related questions

Hello,

Here are some conceptquestions that come from a review for an exam, having some troubleplease help me!!! I know there are multiple questions, Sorry! Ihope someone will help me! be brief but I still want to be able toknow why its that answer! Thanks!

1. What is the purpose of the salt bridge in a galvanic cell? Couldyou have a galvanic cell without it?

2. If a redox reaction involves no net destruction or production ofelectrons, how do we obtain “half cell potentials?”

3. Is E0 positive or negative for an electrolytic cell? For agalvanic cell?

4. A battery is made of two half cells that have a combined E0 of1.8 volts. Is the voltage constant through the life of the battery?Explain why or why not.

5. A galvanic cell is made from a Zn rod in a solution of 1.0 MZnSO4 and a Cu rod in a solution of 1.0 M CuSO4¬. The two cells areconnected with a salt bridge and used to run a small motor. What isthe voltage produced from this cell and which electrodes getsheavier (due to plating of metal) and which electrodes becomeslighter via corrosion. Which electrode is the anode, which is thecathode? You can assume that both half cell reactions involve 2e-.

6. What is the voltage of the cell above if instead, a 0.10 Msolution of ZnSO4 is used? What is the voltage when equilibrium isreached?

7. Using the galvanic system in #7 above, show what happens to thecell voltage as the battery is used. Show what happens withchemical equations and calculate the voltage with the Nernstequation.

8. Explain in detail one of the commercially electrochemicalprocesses described in class. Show the redox equations, explain thetype of electrochem process and explain why this process isindustrially important.



I hope you can HELP!Thanks!

Hello,

Here are some conceptquestions that come from a review for an exam, having some troubleplease help me!!! I know there are multiple questions, Sorry! Ihope someone will help me! be brief but I still want to be able toknow why its that answer! Thanks!

1. What is the purpose of the salt bridge in a galvanic cell? Couldyou have a galvanic cell without it?

2. If a redox reaction involves no net destruction or production ofelectrons, how do we obtain “half cell potentials?”

3. Is E0 positive or negative for an electrolytic cell? For agalvanic cell?

4. A battery is made of two half cells that have a combined E0 of1.8 volts. Is the voltage constant through the life of the battery?Explain why or why not.

5. A galvanic cell is made from a Zn rod in a solution of 1.0 MZnSO4 and a Cu rod in a solution of 1.0 M CuSO4¬. The two cells areconnected with a salt bridge and used to run a small motor. What isthe voltage produced from this cell and which electrodes getsheavier (due to plating of metal) and which electrodes becomeslighter via corrosion. Which electrode is the anode, which is thecathode? You can assume that both half cell reactions involve 2e-.

6. What is the voltage of the cell above if instead, a 0.10 Msolution of ZnSO4 is used? What is the voltage when equilibrium isreached?

7. Using the galvanic system in #7 above, show what happens to thecell voltage as the battery is used. Show what happens withchemical equations and calculate the voltage with the Nernstequation.

8. Explain in detail one of the commercially electrochemicalprocesses described in class. Show the redox equations, explain thetype of electrochem process and explain why this process isindustrially important.



I hope you can HELP!Thanks!

How do you do the math for this? I know cost of Zinc is $5.30/100 g, Silver is $0.56/g, and Lead is $2.45/100g..

The construction of a cell with maximum voltage

Use metal strips and solutions of your choice to determine which combination will give the largest potential. Several different metals and metal salt solutions will be available. In general, the solid metal should be the same metal as that in the salt solution it is in contact with. Utilize a table of standard reduction potentials to help decide which cells to construct. Keep in mind that you can connect more than one cell together. You can also vary the concentration of the metal salt solutions. A minimum of 3 different batteries should be made and tested. Your grade will not be based solely on the number of batteries you make, but also on the strategy used for choosing battery designs and the thoroughness of your investigation. In addition to finding the highest voltage you can achieve, determine which battery gives you the best ratio of volts to cost (V/$).

Battery 1.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Zn2+ (aq) and Zn (s) observed potential = + 1.12 V

Battery 2.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Ag+ (aq) and Ag (s) observed potential = + 2.39 V

Battery 3.) HALF CELL ONE: 1.0 Mg2+ (aq) and 1.0 Mg (s) HALF CELL TWO: 1.0 M Pb2+ (aq) and Pb (s) observed potential = + 1.42 V

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