a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of current pass through an electrolytic cell with an NiNO3 electrode solution for 5.00 hours? Faraday’s Constant = 96,500 Coul/mol e- Ni+(aq) + e- ---->Ni (s) b) To plate a dental explorer with 10.00 g of Nickel (58.6934 g/mol) from a NiNO3 aqueous solution, a metallurgist utilized a 5.00 amp current. How long will it take in minutes, to plate out 10.00 g of zinc? Ni+(aq) + e---->Ni (s)
a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of current pass through an electrolytic cell with an NiNO3 electrode solution for 5.00 hours? Faraday’s Constant = 96,500 Coul/mol e-
Ni+(aq) + e- ---->Ni (s)
b) To plate a dental explorer with 10.00 g of Nickel (58.6934 g/mol) from a NiNO3 aqueous solution, a metallurgist utilized a 5.00 amp current. How long will it take in minutes, to plate out 10.00 g of zinc? Ni+(aq) + e---->Ni (s)
Electrolyte is a material which if dissolved into a polar solvent, generates an electrically conducive solution such as water. The dissolved electrolyte splits into cations and anions that spread the solution equally. This solution is electrically neutral .
Given Nickel is (58.6934 g/mol) plated on to an iron base metal
Current pass through an electrolytic cell is 200.0 Amps
Here time is 5.00 hours
Faraday’s Constant = 96,500 Coul/mol e-
Here equation is
Ni+(aq) + e Ni (s)
2-Given Nickel (58.6934 g/mol) at 10 gm.
Here current is 5.00 amp .
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