# Problem: How many grams of Cu metal (63.55 g/mol) will be plated out of a Cu(NO3 )2 solution by passing a current of 3.00 amperes for 11 minutes? (1 Faraday = 96,485 Coulombs)1. 2.608 g2. 0.652 g 3. 1.304 g4. 0.0721 g

91% (47 ratings)
###### FREE Expert Solution

We’re being asked to calculate the mass of Cu metal plated out of a Cu(NO3)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:

91% (47 ratings)
###### Problem Details

How many grams of Cu metal (63.55 g/mol) will be plated out of a Cu(NO)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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Faraday's Constant concept. You can view video lessons to learn Faraday's Constant. Or if you need more Faraday's Constant practice, you can also practice Faraday's Constant practice problems.

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Our tutors rated the difficulty ofHow many grams of Cu metal (63.55 g/mol) will be plated out ...as medium difficulty.

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