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Solid silver oxide, decomposes at temperatures in excess

General Chemistry: Principles and Modern Applications | 10th Edition | ISBN: 9780132064521 | Authors: Ralph Petrucci ISBN: 9780132064521 175

Solution for problem 24 Chapter 4

General Chemistry: Principles and Modern Applications | 10th Edition

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General Chemistry: Principles and Modern Applications | 10th Edition | ISBN: 9780132064521 | Authors: Ralph Petrucci

General Chemistry: Principles and Modern Applications | 10th Edition

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Problem 24

Solid silver oxide, decomposes at temperatures in excess of 300 C, yielding metallic silver and oxygen gas. A 3.13 g sample of impure silver oxide yields 0.187 g What is the mass percent in the sample? Assume that is the only source of [Hint: Write a balanced equation for the reaction.] O2(g).

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Chem 111 Notes: ch.3 3/1 Stoichiometry­ the study of the quantitative relationships involving the substances in chemical reactions. Chemical equation­ An equation that describes the identities and relative amounts of reactants and products in a chemical reaction. Reactants­ The substances consumed Products­ The substances formed. Coefficients­ Numbers before the formula of a substance in an equation. ­ Balanced equations are equations with the same number of atoms in each element in both the beginning and the end. To wrie a correct formula for an equation… ­ Write the correct formula for each substance ­ Add coefficients so the number of atoms are balanced on both sides of the equation. o If a fractional coefficient is received, mul

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Chapter 4, Problem 24 is Solved
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Textbook: General Chemistry: Principles and Modern Applications
Edition: 10
Author: Ralph Petrucci
ISBN: 9780132064521

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Solid silver oxide, decomposes at temperatures in excess