In an Electroplating Process, It Is Desired to Deposit $40 \mathrm { mg }$

In an electroplating process, it is desired to deposit $40 \mathrm { mg }$ of silver on a metal part by using a current of $2.0 \mathrm {~A}$ . How long must the current be allowed to run to deposit this much silver? The silver ions are singly charged, and the atomic mass of silver is $108 \mathrm {~g} / \mathrm { mol } . \left( e = 1.60 \times 10 ^ { - 19 } \mathrm { C } _ { \mathrm { A } } = \right.$ $6.02 \times 10 ^ { 23 }$ atoms $/ \mathrm { mol }$ )

A) $20 \mathrm {~s}$
B) $18 \mathrm {~s}$
C) $16 \mathrm {~s}$
D) $22 \mathrm {~s}$