First, how much Ag must be deposited? The volume is 30 cm^2 x 0.020 cm = 0.6 cc. mass Ag = volume x density = 0.6 cc x 10.5 g/cc = 6.3 g
You know that 96,485 coulombs will deposit 107.9 g Ag so how many coulombs do you need? That's 96,485 coulombs x (6.3/107.9) = 5,634 C
C =amperes x seconds
5634 C = 4.0 x seconds.
Solve for seconds and convert to hours.
Using a current of 4.0A, how many hours would it take to deposit a silver using coating of 0.2mm thick on a metal with a surface area of 30cm^2 during electrolysis of Ag(CN)2. Given that the density of silver is 10.5g/cm^3
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