What mass of silver would plate onto the cathode if a current of 5.8 A flowed through the cell for 50 min? ?
Silver can be electroplated at the cathode of an electrolysis cell by the following half-reaction.
Ag^+ e^- ----> Ag (s)
What mass of silver would plate onto the cathode if a current of 5.8 A flowed through the cell for 50 min?
t = 50 x 60 = 3000 s
5.8 a for 3000 s is
5.8 coulomb / s x 3000 s = 17400 coulombs
17400 / 96500 = 0.180 faradays
0.180 faradays ( 1 moles Ag / 1 Faraday) = 0.180 mol
mass = 0.180 mol x 107.868 g/mol =19.4 g
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