The decomposition of a silver oxide sample forms 15.8 g of

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

Problem 109P Chapter 11

Introductory Chemistry | 5th Edition

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

Introductory Chemistry | 5th Edition

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Problem 109P

PROBLEM 109P

The decomposition of a silver oxide sample forms 15.8 g of Ag(s):

2 Ag2O(s) → 4Ag(s) + O2(g)

What total volume of O2 gas forms if it is collected over water at a temperature of 25 °C and a total pressure of 752 mm Hg?

Step-by-Step Solution:
Step 1 of 3

Solution 109P

Given that

Your reaction will produce 0.94 L of oxygen gas.

The first thing you need to do is determine how many moles of oxygen gas are produced when that much silver is produced. To do this, use the number of moles of silver and the mole ratio that exists between the two products.

2Ag2O(s)→4Ag(s)+O2(g)

Notice that you have a 4:1 mole ratio between silver and oxygen, which means that you get 1 mole of oxygen for every 4 moles of silver produced.

The number of moles of silver the reaction produced is

15.9g⋅1 mole Ag/107.87g=0.1474 moles Ag.

This means that you'll get

0.1474moles Ag/1...

Step 2 of 3

Chapter 11, Problem 109P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo Tro
ISBN: 9780321910295

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