A Jeweler Needs to Electroplate Gold, Having an Atomic Mass $196.97 \mathrm {~g} / \mathrm { mol }$

A jeweler needs to electroplate gold, having an atomic mass of $196.97 \mathrm {~g} / \mathrm { mol }$ , onto a bracelet. He knows that the charge carriers in the ionic solution are singly-ionized gold ions, $\mathrm { Au } ^ { + }$ , and has calculated that he must deposit $0.20 \mathrm {~g}$ of gold to reach the necessary thickness. How much current does he need to plate the bracelet in $3.0$ hours? $\left( e = 1.60 \times 10 ^ { - 19 } \mathrm { C } , \mathrm { N } _ { \mathrm { A } } = 6.02 \times 10 ^ { 23 } \right.$ atoms/mol)

A) $540 \mathrm {~mA}$
B) $33 \mathrm {~A}$
C) $1800 \mathrm {~mA}$
D) $9.1 \mathrm {~mA}$