Q1. What is the cell potential of a galvanic cell with E° = 1.5 V and Q = 10?
Solution:
Using the Nernst equation, E = E° - (RT/nF)lnQ, we find E ≈ 1.0 V.
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Q2. In electrolysis, the process of oxidation occurs at the: (2023)
Solution:
In electrolysis, oxidation occurs at the anode.
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Q3. What is the Nernst equation for a cell at 298 K with E° = 0.77 V and [Zn²⁺] = 0.01 M?
Solution:
Using the Nernst equation: E = E° - (0.0591/n) log([Zn²⁺]), where n=2.
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Q4. In electrolysis, if the current is 2 A and the time is 30 minutes, how many moles of electrons are transferred?
Solution:
Using the formula: moles = (current × time) / (n × F), where n=1 for electrons and F=96500 C/mol.
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Q5. What is the Nernst equation used for calculating the cell potential at non-standard conditions? (2023)
Solution:
The Nernst equation is E = E° - (RT/nF)lnQ, where E is the cell potential, E° is the standard potential, R is the gas constant, T is the temperature, n is the number of moles of electrons, and F is Faraday's constant.
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Q6. Which of the following is a primary cell? (2023) 2023
Solution:
The zinc-carbon battery is a type of primary cell, which cannot be recharged.
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Q7. In electrolysis, the process of oxidation occurs at the: (2023) 2023
Solution:
In electrolysis, oxidation occurs at the anode.
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Q8. 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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Q9. If the concentration of Cu²⁺ in a cell is increased, what happens to the cell potential?
Solution:
Increasing the concentration of Cu²⁺ increases the cell potential according to the Nernst equation.
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Q10. What is the product of electrolysis of water?
Solution:
The products of electrolysis of water are hydrogen and oxygen.
