Suppose that gold is being plated on to another metal in an electrolytic cell. The half-cell reaction producing the Au ( s ) is AuCl 4 - arrow Au (s)+4 Cl --3 e- If a 0.30 A current runs for 15.00 min, what mass of Au (s) will be plated, assuming all the electrons are used in the reduction of AuCl 4-? The Faraday constant is 96485 C / mol and molar mass of Au is 197 .

Question

Suppose that gold is being plated on to another metal in an electrolytic cell. The half-cell reaction producing the Au ( s ) is AuCl 4 - arrow Au (s)+4 Cl --3 e- If a 0.30 A current runs for 15.00 min, what mass of Au (s) will be plated, assuming all the electrons are used in the reduction of AuCl 4-? The Faraday constant is 96485 C / mol and molar mass of Au is 197 . (A) 0.184 g Au (B) 0.551 g Au (C) 1.84 g Au (D) 0.613 g Au

Tardigrade Admin · Accepted Answer

Mass of Au deposited = Number of Faraday passed × Eq. mass =(0.30 × 15 × 60/96485) × (197/3) =0.184 g

0.184 g Au

0.551 g Au

1.84 g Au

0.613 g Au

Mass of Au deposited = Number of Faraday passed × Eq. mass =964850.30×15×60​×3197​ =0.184g

Mass of $A u$ deposited $=$ Number of Faraday passed $\times$ Eq. mass
$= \frac{0.30 \times 15 \times 60}{96485} \times \frac{197}{3}$
$= 0.184 g$