Calculate the mass of copper deposited when a c... - JAMB Chemistry 2017 Question
Calculate the mass of copper deposited when a current of 0.5 ampere was passed through a solution of copper(II) chloride for 45 minutes in an electrolytic cell. [Cu = 64, F = 96500Cmol-1]
A
0.300g
B
0.250g
C
0.2242g
D
0.448g
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Correct Option: D
M = (\frac{\text{Molar mass × Quantity of Electricity}}{\text{96500 × no of charge}})
= (\frac{MmIT}{96500n})
Copper II Chloride = CuCl2
CuCl2 → Cu2+ + 2Cl2
Mass of compound deposited = (\frac{\text{Molar mass × Quantity of Electricity}}{\text{96500 × no of charge}})
Q = IT
I = 0.5A
T = 45 × 60
T = 2700s
Q = 0.5 × 2700
= 1350c
Molarmass = 64gmol-1
no of charge = + 2
Mass = (\frac{64 \times 1350}{96500 \times 2})
Mass = 0.448g
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