Question

ere: 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

Answer 1

Answer: 8.95 hours

Explanation:

$Ni^{2+}+2e^-\rightarrow Ni$

$96500\times 2=193000$ 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 =$\frac{193000}{58.7}\times 1000=3287904.6C$  of electricity

$Q=I\times t$

where Q= quantity of electricity in coloumbs  = 3287904.6C

I = current in amperes = 102 A

t= time in seconds = ?

$3287904.6C=102A\times t$

$t=32234.359sec$

$t=8.95hr$      (1h=3600 sec)

Thus 8.95 hours it takes to plate out 1.0 kg Ni from aqueous $Ni^{2+}$ solution, if the electrical current is 102 A.