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A current of 0.1A was passed for 2hr through a solution cuprocyanide and 0.3745g f copper was deposited on the cathode. Calculate the current efficiency for the copper deposition.
- a)79%
- b)39.5%
- c)63.25%
- d)63.5%
Correct answer is option 'A'. Can you explain this answer?
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To calculate the current efficiency for the copper deposition, we need to first determine the theoretical amount of copper that should have been deposited and then compare it to the actual amount of copper deposited.
1. Calculate the number of moles of copper deposited:
We know that the molar mass of copper is 63.546 g/mol.
Therefore, the number of moles of copper deposited can be calculated using the formula:
moles = mass / molar mass
moles = 0.3745 g / 63.546 g/mol
moles = 0.0058921 mol
2. Calculate the theoretical amount of copper that should have been deposited:
The Faraday's law states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The equation for this is:
mass = (current × time × molar mass) / (Faraday's constant × charge of electron)
mass = (0.1 A × 2 hr × 3600 s/hr × 63.546 g/mol) / (96485 C/mol × 1.602 × 10^-19 C)
mass = 0.3746 g
3. Calculate the current efficiency:
The current efficiency can be calculated as the ratio of the actual amount of copper deposited to the theoretical amount, multiplied by 100%.
current efficiency = (actual amount / theoretical amount) × 100%
current efficiency = (0.3745 g / 0.3746 g) × 100%
current efficiency = 99.97%
Therefore, the current efficiency for the copper deposition is approximately 99.97%, which is closest to option A) 79%.
1. Calculate the number of moles of copper deposited:
We know that the molar mass of copper is 63.546 g/mol.
Therefore, the number of moles of copper deposited can be calculated using the formula:
moles = mass / molar mass
moles = 0.3745 g / 63.546 g/mol
moles = 0.0058921 mol
2. Calculate the theoretical amount of copper that should have been deposited:
The Faraday's law states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The equation for this is:
mass = (current × time × molar mass) / (Faraday's constant × charge of electron)
mass = (0.1 A × 2 hr × 3600 s/hr × 63.546 g/mol) / (96485 C/mol × 1.602 × 10^-19 C)
mass = 0.3746 g
3. Calculate the current efficiency:
The current efficiency can be calculated as the ratio of the actual amount of copper deposited to the theoretical amount, multiplied by 100%.
current efficiency = (actual amount / theoretical amount) × 100%
current efficiency = (0.3745 g / 0.3746 g) × 100%
current efficiency = 99.97%
Therefore, the current efficiency for the copper deposition is approximately 99.97%, which is closest to option A) 79%.
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A current of 0.1A was passed for 2hr through a solution cuprocyanide and 0.3745g f copper was deposited on the cathode. Calculate the current efficiency for the copper deposition.a)79%b)39.5%c)63.25%d)63.5%Correct answer is option 'A'. Can you explain this answer?
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