We’re being asked to calculate the mass of Cu metal plated out of a Cu(NO3)2 solution.
• 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:
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 g
2. 0.652 g
3. 1.304 g
4. 0.0721 g
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