How long of time in hours will it take to plate out 1.0 kg ni from aqueous ni2+ solution, if the electrical current is 102 a? where: ni2+(aq)+2e-→ni(s) view available hint(s) how long of time in hours will it take to plate out 1.0 kg ni from aqueous ni2+ solution, if the electrical current is 102 a? where: ni2+(aq)+2e-→ni(s) 90 hours 0.895 hours 8.95 hours 900 hours

8.95 hours

Explanation:

Coloumb of electricity deposits 1 mole of Nickel

1 mole of Nickel weighs = 58.7 g

Given quantity = 1.0 kg = 1000 g  (1kg=1000g)

58.7 g of Nickel is deposited by 193000 C of electricity

1000 g of Nickel is deposited by =  of electricity

where Q= quantity of electricity in coloumbs  = 3287904.6C

I = current in amperes = 102 A

t= time in seconds = ?

     (1h=3600 sec)

Thus 8.95 hours it takes to plate out 1.0 kg Ni from aqueous solution, if the electrical current is 102 A.

what is the question here. i think you messed up.