How long does it take to electroplate 0.5 mm of gold on an object with a surface area of 31 cm^^ from an Au3+(aq) solution with a 8 A current? Recall the density of gold is 19.3 g/cm^3.

It will take 5492 seconds to electroplate 0.5 mm of gold on an object .

Explanation:

Mass of gold = m

Volume of gold = v

Surface area on which gold is plated =

Thickness of the gold plating  = h = 0.5 mm = 0.05 cm

1 mm = 0.1 cm

Density of the gold =

Moles of gold =

According to reaction, 1 mole of gold required 3 moles of electrons,then 0.152 moles of gold will require :

of electrons

Number of electrons = N =

Charge on single electron =

Total charge required = Q

Amount of current passes = I = 8 Ampere

Duration of time  = T

It will take 5492 seconds to electroplate 0.5 mm of gold on an object .