Question

80.1% Resources Hint An object with a surface area of 61.5 cm is to be plated with nickel. A current of 8.03 A is applied to a solution containing nickel in the +2 oxidation state. Calculate the time required to coat the object with an even layer of nickel that is 5.93 x 10-3 cm thick. The density of nickel is 8.91 g/cm'. time: about us Careers privacy policy Terms of use contact us help 39% ^ ( od

Answer 1

Volume of the object required to coat

= surface area $\small \times$ thickness

= 61.5 (cm²) $\small \times$ 5.93$\small \times$10^-3 (cm)

= 0.365 cm³

Mass of Ni deposited

= volume of the object required to coat  $\small \times$density of Ni

= 0.365 (cm³)  $\small \times$ 8.91(g/cm³)

= 3.25 g.

By Faraday law of electrolysis

W =

Exixt

charge of Ni ( n factor) = +2

E is gm equivalent of Ni = ( atomic mass/ n factor) = (58.7/2)

= 29.35 g

W is mass of Ni deposited

= 3.25 g

i is current = 8.03 A

F = 96500 C

t is time in sec .

so, time required (t) to coat the object

t =

W XF iXE

t = ( 3.25$\small \times$96500/ 8.03$\small \times$29.35)

t = 1331 s .