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Chemistry / Introductory Chemistry 5 / Chapter 16 / Problem 103P

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

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

Chapter 16, Problem 103P

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QUESTION:

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

\(\mathrm{Ag}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)\)

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

Questions & Answers

QUESTION:

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

\(\mathrm{Ag}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)\)

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

ANSWER:

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 $\frac{1\ mol}{107.868\ g}$

= 0.0537 mol

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