Textbook Question
Balance the following equations:
(a) HClO4(aq) + P4O10(s) → HPO3(aq) + Cl2O7(l)
(b) Au2S3(s + H2(g) → Au(s) + H2S(g)
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 3, Problem 10
A key step in balancing chemical equations is correctly identifying the formulas of the reactants and products. For example, consider the reaction between calcium oxide, CaO(s), and H2O1l2 to form aqueous calcium hydroxide. (b) Is it possible to balance the equation if you incorrectly identify the product as CaOH1aq2, and if so, what is the equation?
Verified step by step guidance1
Identify the correct chemical formulas for the reactants and the incorrectly identified product: CaO(s), H_2O(l), and CaOH(aq).
Write the unbalanced chemical equation using these formulas: CaO(s) + H_2O(l) \(\rightarrow\) CaOH(aq).
Count the number of each type of atom on both sides of the equation. For the reactants, you have 1 Ca, 1 O, and 2 H atoms. For the product, you have 1 Ca, 1 O, and 1 H atom.
To balance the equation, adjust the coefficients to ensure the same number of each type of atom appears on both sides. Since the product has only 1 H atom, you need to balance the hydrogen atoms by adjusting the coefficient of H_2O.
Re-evaluate the equation after adjusting coefficients to ensure all atoms are balanced, and verify that the equation is consistent with the law of conservation of mass.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Chemical Formulas
Chemical formulas represent the composition of substances, indicating the types and numbers of atoms present. Accurate identification of reactants and products is crucial in chemical reactions, as incorrect formulas can lead to misunderstandings in the reaction process and the final balanced equation.
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Skeletal Formula
Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. An incorrect product formula can complicate this process, potentially leading to an unbalanced equation.
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Hydroxide Ion Formation
In the context of the reaction between calcium oxide and water, the formation of hydroxide ions (OH-) is essential. The correct product, calcium hydroxide (Ca(OH)2), contains two hydroxide ions, which are crucial for the compound's properties. Misidentifying the product as CaOH could lead to confusion regarding the stoichiometry and the resulting chemical behavior.
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Related Practice
Textbook Question
Write 'true' or 'false' for each statement. (a) We balance chemical equations as we do because energy must be conserved.
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Textbook Question
Write 'true' or 'false' for each statement. (b) If the reaction 2 O3(g) → 3 O2(g) goes to completion and all O3 is converted to O2, then the mass of O3 at the beginning of the reaction must be the same as the mass of O2 at the end of the reaction.
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Textbook Question
Balance the following equations: (c) Al(OH)3(s) + H2SO4(l) → Al2(SO4)3(s) + H2O(l)
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Textbook Question
Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over?
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