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Q1. Which of the following statements is true about galvanic cells? (2020)
Solution:
Galvanic cells convert chemical energy into electrical energy spontaneously.
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Q2. In electrolysis, if 1 mole of electrons is transferred, how many grams of copper can be deposited from Cu²⁺?
Solution:
1 mole of Cu²⁺ deposits 63.5 g of copper.
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Q3. What is the standard electrode potential of the half-reaction Zn²⁺ + 2e⁻ → Zn?
Solution:
The standard electrode potential for Zn²⁺/Zn is -0.76 V.
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Q4. What is the relationship between Gibbs free energy (ΔG) and cell potential (E) in electrochemistry?
Solution:
The relationship is ΔG = -nFE, where n is the number of moles of electrons transferred.
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Q5. What is the standard electrode potential of the hydrogen electrode? (2023) 2023
Solution:
The standard electrode potential of the hydrogen electrode is defined as 0 V.
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Q6. What is the cell potential of a Daniell cell at standard conditions?
Solution:
The standard cell potential of a Daniell cell is 1.10 V.
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Q7. What is the Faraday's constant value?
Solution:
Faraday's constant is approximately 96485 C/mol.
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Q8. In a galvanic cell, if the anode reaction is Zn → Zn²⁺ + 2e⁻, what is the cathode reaction if the cathode is Cu²⁺ + 2e⁻ → Cu?
Solution:
The cathode reaction is Cu²⁺ + 2e⁻ → Cu.
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Q9. In a galvanic cell, if the anode reaction is Ag⁺ + e⁻ → Ag, what is the cathode reaction?
Solution:
The cathode reaction must be a reduction; Ag⁺ + e⁻ → Ag is the anode reaction.
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Q10. In a Daniell cell, which metal acts as the anode?
Solution:
In a Daniell cell, Zinc acts as the anode.
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