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Calculate the mass of cu deposited when a current of 0.45 ampere passing through CuSO4 for 1hr 15mins
Accepted Answer
The mass of copper deposited (w) can be calculated using Faraday's law of electrolysis:
w = (Q * M) / (z * F)
where:
- w is the mass of the substance deposited (in grams)
- Q is the quantity of charge passed through the solution (in Coulombs)
- M is the molar mass of the substance being deposited (in grams per mole)
- z is the number of electrons transferred per mole of the substance being deposited
- F is the Faraday constant (96,485 Coulombs per mole of electrons)
Given:
- Current (I) = 0.45 A
- Time (t) = 1 hour 15 minutes = 75 minutes = 4500 seconds
- Molar mass of Cu (M) = 63.55 g/mol
- z = 2 (for Cu2+ ions)
Calculate the charge passed through the solution (Q):
Q = I * t
= 0.45 A * 4500 s
= 2025 C
Now, calculate the mass of Cu deposited (w):
w = (Q * M) / (z * F)
= (2025 C * 63.55 g/mol) / (2 * 96485 C/mol)
= 0.698 grams
Therefore, the mass of Cu deposited is 0.698 grams.
w = (Q * M) / (z * F)
where:
- w is the mass of the substance deposited (in grams)
- Q is the quantity of charge passed through the solution (in Coulombs)
- M is the molar mass of the substance being deposited (in grams per mole)
- z is the number of electrons transferred per mole of the substance being deposited
- F is the Faraday constant (96,485 Coulombs per mole of electrons)
Given:
- Current (I) = 0.45 A
- Time (t) = 1 hour 15 minutes = 75 minutes = 4500 seconds
- Molar mass of Cu (M) = 63.55 g/mol
- z = 2 (for Cu2+ ions)
Calculate the charge passed through the solution (Q):
Q = I * t
= 0.45 A * 4500 s
= 2025 C
Now, calculate the mass of Cu deposited (w):
w = (Q * M) / (z * F)
= (2025 C * 63.55 g/mol) / (2 * 96485 C/mol)
= 0.698 grams
Therefore, the mass of Cu deposited is 0.698 grams.
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