Ag+ + 1e- → Ag(s)
• current = 2.00 A
• time = 2.30 min (convert to from min to s)
• Faraday’s constant = 96485 C/(mol e-)
• From the reaction: 1 mol e- produces 1 mol Ag(s)
It took 2.30 min using a current of 2.00 A to plate out all the silver from 0.250 L of a solution containing Ag +. What was the original concentration of Ag + in the solution?
Frequently Asked Questions
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 Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.