question_answer

Suppose that gold is being plated on to another metal in an electrolytic cell. The half-cell reaction    producing    the   Au(s) is\[\frac{x+2}{6}=\frac{y-4}{3}=\frac{z+1}{2}\] lf 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 \[\frac{x+2}{-6}=\frac{y-4}{3}=\frac{z+1}{2}\] ? 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