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The amount of electricity required to produce one mole of copper from copper sulphate solution will be:
- a)1 faraday
- b)2.33 faraday
- c)2 faraday
- d)1.33 faraday
Correct answer is option 'C'. Can you explain this answer?
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The amount of electricity required to produce one mole of copper from ...
no. of electrons used is equal to no. of Faradays.Most Upvoted Answer
The amount of electricity required to produce one mole of copper from ...
Explanation:
To understand why the correct answer is option 'C', let's break down the process of copper electrodeposition from copper sulphate solution and calculate the amount of electricity required.
1. Electrolysis of Copper Sulphate Solution:
When a copper sulphate solution is electrolyzed using a copper electrode as the cathode, copper ions (Cu2+) from the solution are reduced and deposited onto the cathode as solid copper. The overall reaction can be represented as follows:
Cu2+ + 2e- → Cu(s)
2. Faraday's Law of Electrolysis:
Faraday's law of electrolysis states that the amount of substance deposited or liberated at an electrode during electrolysis is directly proportional to the quantity of electric charge passed through the electrolyte. The relationship is given by the equation:
Q = n × F
Where:
- Q is the quantity of electric charge (in coulombs)
- n is the number of moles of substance deposited or liberated
- F is Faraday's constant, which is equal to the charge of one mole of electrons (approximately 96,485 C/mol)
3. Calculation:
To determine the amount of electricity required to produce one mole of copper, we need to calculate the quantity of electric charge (Q) required.
From the balanced reaction, we can see that 2 moles of electrons (2e-) are required to reduce one mole of copper ions (Cu2+). Therefore, n = 1 mole.
Using Faraday's law, we can rearrange the equation to solve for Q:
Q = n × F
Q = 1 mole × 96,485 C/mol
Q = 96,485 C
Therefore, the amount of electricity required to produce one mole of copper is 96,485 coulombs, which is equal to 1 Faraday. Thus, the correct answer is option 'C'.
To understand why the correct answer is option 'C', let's break down the process of copper electrodeposition from copper sulphate solution and calculate the amount of electricity required.
1. Electrolysis of Copper Sulphate Solution:
When a copper sulphate solution is electrolyzed using a copper electrode as the cathode, copper ions (Cu2+) from the solution are reduced and deposited onto the cathode as solid copper. The overall reaction can be represented as follows:
Cu2+ + 2e- → Cu(s)
2. Faraday's Law of Electrolysis:
Faraday's law of electrolysis states that the amount of substance deposited or liberated at an electrode during electrolysis is directly proportional to the quantity of electric charge passed through the electrolyte. The relationship is given by the equation:
Q = n × F
Where:
- Q is the quantity of electric charge (in coulombs)
- n is the number of moles of substance deposited or liberated
- F is Faraday's constant, which is equal to the charge of one mole of electrons (approximately 96,485 C/mol)
3. Calculation:
To determine the amount of electricity required to produce one mole of copper, we need to calculate the quantity of electric charge (Q) required.
From the balanced reaction, we can see that 2 moles of electrons (2e-) are required to reduce one mole of copper ions (Cu2+). Therefore, n = 1 mole.
Using Faraday's law, we can rearrange the equation to solve for Q:
Q = n × F
Q = 1 mole × 96,485 C/mol
Q = 96,485 C
Therefore, the amount of electricity required to produce one mole of copper is 96,485 coulombs, which is equal to 1 Faraday. Thus, the correct answer is option 'C'.
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