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Gold 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 104P 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 104P

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

Au3+(aq) + 3e‑ → Au(s)

How many moles of electrons are required to electroplate 1.40 g of Au?

Step-by-Step Solution:

Solution 104 P:

Here, we are going to calculate the moles of electrons are required to electroplate of 1.40 g of Au.

Step 1:

 Molar mass of Au  =196.96 g/mol

Amount of Au required  to electroplate 5.8 g of Au  = 1.40 g Au x

                                                    = 0.0071 mol

Step 2 of 2

Chapter 16, Problem 104P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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