Practice Electrochemical Cells And Standard Electrode Potentials (3) - Unit 9: Redox Processes

Practice: Electrochemical Cells and Standard Electrode Potentials

Lesson 3Unit 9: Redox Processes

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6 sample questions

Question 1.
What is the main function of a galvanic cell?
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Consider the type of energy transformation.
Question 2.
What does the anode represent in a galvanic cell?
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Think about where electrons are released.
3Question 3.
What does a positive cell potential imply?
- The reaction is non-spontaneous
- The reaction is spontaneous
- The reaction does not occur
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Think about how energy transformations lead to spontaneous behavior.
4Question 4.
True or False: The anode is where reduction occurs.
- True
- False
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Recall 'Red Cat' and 'An Ox' for identifying electrode behaviors.
Question 5.
Determine the standard cell potential for a galvanic cell consisting of a silver half-cell (Ag⁺ + e⁻ → Ag) with E° = +0.80 V and a zinc half-cell (Zn²⁺ + 2e⁻ → Zn) with E° = -0.76 V.
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Identify which is oxidized and which is reduced.
Question 6.
What would happen to the cell potential if the concentration of Cu²⁺ is increased significantly in a copper-zinc galvanic cell?
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Recall how concentration affects the reaction quotient in the Nernst equation.

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