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The density of copper is 8.94 g/L find the charge needed to plate an area of 10 x 10cm2 to a thickness
of 10-2 to a thickness of CuSo4 solution as electrolyte(At.wt of Cu = 63.6)
of 10-2 to a thickness of CuSo4 solution as electrolyte(At.wt of Cu = 63.6)
- a)2.7 x 104 C
- b)8.8 x 104 C
- c)18.3 x 104C
- d)104C
Correct answer is option 'A'. Can you explain this answer?
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The density of copper is 8.94 g/L find the charge needed to plate an a...
Calculate the density of copper with area
and thickness of CuSo4 as CU=63.6
A is correct by calculate the area
and thickness of CuSo4 as CU=63.6
A is correct by calculate the area
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Community Answer
The density of copper is 8.94 g/L find the charge needed to plate an a...
Calculation of the charge needed to plate copper
Given data:
- Density of copper = 8.94 g/L
- Area to be plated = 10 x 10 cm² = 100 cm²
- Thickness of plating = 10^-2 cm
- Atomic weight of copper (Cu) = 63.6 g/mol
Calculations:
1. Calculate the volume of copper required for plating:
Volume = Area x Thickness
Volume = 100 cm² x 10^-2 cm
Volume = 1 cm³
2. Calculate the mass of copper required:
Mass = Density x Volume
Mass = 8.94 g/L x 1 cm³
Mass = 8.94 g
3. Calculate the number of moles of copper required:
Moles = Mass / Atomic weight
Moles = 8.94 g / 63.6 g/mol
Moles = 0.1405 mol
4. Calculate the charge needed to plate this amount of copper:
As 1 mol of electrons corresponds to 1 mole of Cu, the charge required is equal to the number of moles of Cu.
Charge = 0.1405 mol x 1 F
Charge = 0.1405 F
Final answer:
The charge needed to plate an area of 10 x 10 cm² to a thickness of 10^-2 cm in a CuSO4 solution as an electrolyte is 2.7 x 10^4 C. Hence, option 'A' is correct.
Given data:
- Density of copper = 8.94 g/L
- Area to be plated = 10 x 10 cm² = 100 cm²
- Thickness of plating = 10^-2 cm
- Atomic weight of copper (Cu) = 63.6 g/mol
Calculations:
1. Calculate the volume of copper required for plating:
Volume = Area x Thickness
Volume = 100 cm² x 10^-2 cm
Volume = 1 cm³
2. Calculate the mass of copper required:
Mass = Density x Volume
Mass = 8.94 g/L x 1 cm³
Mass = 8.94 g
3. Calculate the number of moles of copper required:
Moles = Mass / Atomic weight
Moles = 8.94 g / 63.6 g/mol
Moles = 0.1405 mol
4. Calculate the charge needed to plate this amount of copper:
As 1 mol of electrons corresponds to 1 mole of Cu, the charge required is equal to the number of moles of Cu.
Charge = 0.1405 mol x 1 F
Charge = 0.1405 F
Final answer:
The charge needed to plate an area of 10 x 10 cm² to a thickness of 10^-2 cm in a CuSO4 solution as an electrolyte is 2.7 x 10^4 C. Hence, option 'A' is correct.
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The density of copper is 8.94 g/L find the charge needed to plate an area of 10 x 10cm2to a thicknessof 10-2to a thickness of CuSo4solution as electrolyte(At.wt of Cu = 63.6)a)2.7 x 104 Cb)8.8 x 104 Cc)18.3 x 104Cd)104CCorrect answer is option 'A'. Can you explain this answer?
Question Description
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