🤓 Based on our data, we think this question is relevant for Professor Delgado's class at FIU.

How many grams of Cu metal (63.55 g/mol) will be plated out of a Cu(NO_{3 })_{2} solution by passing a current of 3.00 amperes for 11 minutes? (1 Faraday = 96,485 Coulombs)

1. 2.608 g

2. 0.652 g

3. 1.304 g

4. 0.0721 g

We’re being asked to calculate the mass of Cu metal plated out of a Cu(NO_{3})_{2} solution.

**Given:**

•** molar mass Cu = 63.55 g/mol**

• **current = 3.00 A**** **▪ *Note that amperes (A) = charge/time = C/s** *▪ **Current = 3.00 C/s**

•** t = 11 minutes**** **▪ *Since the current is in C/ s, we will have to convert time from min to s*

•** Faraday’s constant = 96,485 C/(mol e ^{-})**

Let’s first determine **how many electrons** are involved when Cu is plated out from the solution:

Faraday's Constant

Faraday's Constant

Faraday's Constant

Faraday's Constant