How much time would be needed to deposit 0.25 g of metallic nickel. (Atomic mass = 58.5) on a metal object using a current of 1A during electroplating?

Explanation

`Ni^(++) + 2e^(-) to Ni`
2F or `2 xx 96500` C of electricity is required to deposit 58.5 g of Ni.
58.5 g of Ni requires `2 xx 96500` C
0.25 g Ni requires `=(2 xx 96500 xx 0.25)/58.5 = 824.8` C
Amount of electricity = Current in amperes `xx` time in seconds
Time in seconds `=("Amount of electricity")/("Current in amperes")`
`=824.8/1 = 824.8 sec = 13.74` minutes.