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What to do: Read each statement below and identify if it defines electrode potential, reduction potential, oxidation potential or cell potential. Write your answers on a separate sheet of раper. 1. It refers to the difference of equilibrium potential between the surrounding solution and the metal electrode. 2. It is the reaction that takes place at the cathode. 3. It is the reaction that takes place at the anode. 4. It is the ability of anion solution to become reduced picking up or gaining electrons from its own electrode. 5. It is the ability of an electrode to become oxidized giving up or losing electrons. 6. It refers to the potential difference between the electrodes corresponding to an external electron flow from anode to cathode. 7. It is the combination of reduction potential at the cathode and oxidation potential at the anode. 8. An example of this reaction is Zns) 9. An example of this reaction is Cu*?jaq) + 2e- 10. It is illustrated as: Ecell = Eox,Anode + Ered,Cathode Znaq) + 2e- . » Cus) -

What to do: Read each statement below and identify if it defines electrode potential, reduction potential, oxidation potential or cell potential. Write your answers on a separate sheet of раper. 1. It refers to the difference of equilibrium potential between the surrounding solution and the metal electrode. 2. It is the reaction that takes place at the cathode. 3. It is the reaction that takes place at the anode. 4. It is the ability of anion solution to become reduced picking up or gaining electrons from its own electrode. 5. It is the ability of an electrode to become oxidized giving up or losing electrons. 6. It refers to the potential difference between the electrodes corresponding to an external electron flow from anode to cathode. 7. It is the combination of reduction potential at the cathode and oxidation potential at the anode. 8. An example of this reaction is Zns) 9. An example of this reaction is Cu*?jaq) + 2e- 10. It is illustrated as: Ecell = Eox,Anode + Ered,Cathode Znaq) + 2e- . » Cus) -

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 22E: The mass of three different metal electrodes, each from a different galvanic cell, were determined...
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What to do: Read each statement below and identify if it defines electrode potential, reduction potential, oxidation potential or cell potential. Write your answers on a separate sheet of раper. 1. It refers to the difference of equilibrium potential between the surrounding solution and the metal electrode. 2. It is the reaction that takes place at the cathode. 3. It is the reaction that takes place at the anode. 4. It is the ability of anion solution to become reduced picking up or gaining electrons from its own electrode. 5. It is the ability of an electrode to become oxidized giving up or losing electrons. 6. It refers to the potential difference between the electrodes corresponding to an external electron flow from anode to cathode. 7. It is the combination of reduction potential at the cathode and oxidation potential at the anode. 8. An example of this reaction is Zns) 9. An example of this reaction is Cu*?laq) + 2e- 10. It is illustrated as: Ecell = Eox,Anode + Ered,Cathode Znag) + 2e-. » Cus) .
Transcribed Image Text:What to do: Read each statement below and identify if it defines electrode potential, reduction potential, oxidation potential or cell potential. Write your answers on a separate sheet of раper. 1. It refers to the difference of equilibrium potential between the surrounding solution and the metal electrode. 2. It is the reaction that takes place at the cathode. 3. It is the reaction that takes place at the anode. 4. It is the ability of anion solution to become reduced picking up or gaining electrons from its own electrode. 5. It is the ability of an electrode to become oxidized giving up or losing electrons. 6. It refers to the potential difference between the electrodes corresponding to an external electron flow from anode to cathode. 7. It is the combination of reduction potential at the cathode and oxidation potential at the anode. 8. An example of this reaction is Zns) 9. An example of this reaction is Cu*?laq) + 2e- 10. It is illustrated as: Ecell = Eox,Anode + Ered,Cathode Znag) + 2e-. » Cus) .
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