Practice The Nernst Equation For A Half-cell Or Full Cell (8.6.1)

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6 sample questions

Question 1.
What does E° represent in electrochemistry?
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Think about the voltage measured at standard conditions.
Question 2.
What does the variable Q stand for in the Nernst equation?
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Consider the ratio of concentrations in the reaction.
3Question 3.
What does the Nernst equation allow you to predict?
- Concentration of products at standard conditions
- Cell potential under non-standard conditions
- Rate of the reaction
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Think about how electrochemical cells behave beyond standard states.
4Question 4.
If Q < K, what happens to the cell potential?
- True
- False
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Consider what direction the reaction shifts.
Question 5.
Given E° = 0.77 V, T = 298 K, and the reaction 2H⁺ + 2e⁻ ⇌ H₂, calculate the cell cell potential when [H⁺] = 0.01 M.
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First, find Q and remember n for hydrogen is 2.
Question 6.
Calculate the potential for a Daniell cell with E° = 1.10 V, [Zn²⁺] = 0.50 M, and [Cu²⁺] = 4.0 M.
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Make sure to calculate Q correctly!

4 more questions in this section. Enroll free to practise them all.