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Silver is electroplated at the cathode of an electrolysis cell by this

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 103P Chapter 16

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 103P

Silver is electroplated at the cathode of an electrolysis cell by this half-reaction.

Ag+(aq) + e‑ → Ag(s)

How many moles of electrons are required to electroplate 5.8 g of Ag?

Step-by-Step Solution:

Solution 103 P:

Here, we are going to calculate the moles of electrons are required to electroplate of 5.8 g of Ag.

Step 1:

 Molar mass of Ag  =107.868 g/mol

Amount of Ag required  to electroplate 5.8 g of Ag  = 5.8 g Ag x

                                                    = 0.0537 mol

Step 2 of 2

Chapter 16, Problem 103P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Silver is electroplated at the cathode of an electrolysis cell by this