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

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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:

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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

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