Textbook Question
Calculate the percentage by mass of oxygen in the following compounds: (b) isopropyl alcohol, C3H8O
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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 23
Determine the formula weights of each of the following compounds: (a) lead(IV) chloride (b) copper(II) oxide (c) iodic acid, HIO3 (d) sodium perchlorate, NaClO4
Verified step by step guidance1
Step 1: Identify the chemical formula for each compound. For lead(IV) chloride, the formula is PbCl4. For copper(II) oxide, the formula is CuO. For iodic acid, the formula is HIO3. For sodium perchlorate, the formula is NaClO4.
Step 2: Determine the atomic weights of each element involved in the compounds using the periodic table. For example, lead (Pb) has an atomic weight of approximately 207.2 amu, chlorine (Cl) is about 35.45 amu, copper (Cu) is about 63.55 amu, oxygen (O) is about 16.00 amu, iodine (I) is about 126.90 amu, sodium (Na) is about 22.99 amu.
Step 3: Calculate the formula weight for each compound by multiplying the atomic weight of each element by the number of atoms of that element in the formula, and then summing these values. For PbCl4, calculate (1 x 207.2) + (4 x 35.45). For CuO, calculate (1 x 63.55) + (1 x 16.00). For HIO3, calculate (1 x 126.90) + (3 x 16.00). For NaClO4, calculate (1 x 22.99) + (1 x 35.45) + (4 x 16.00).
Step 4: Add the calculated values for each element in the compound to find the total formula weight. This involves summing the products from the previous step for each compound.
Step 5: Review the calculations to ensure accuracy and consistency with the atomic weights and the chemical formulas provided. This step ensures that the formula weights are correctly determined for each compound.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass Calculation
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a chemical formula, taking into account the number of each type of atom present. For example, in lead(IV) chloride (PbCl4), the molar mass is calculated by adding the atomic mass of lead (207.2 g/mol) to four times the atomic mass of chlorine (35.5 g/mol).
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Molar Mass Calculation Example
Chemical Nomenclature
Chemical nomenclature is the system of naming chemical compounds based on their composition and structure. It follows specific rules set by organizations like IUPAC. For instance, lead(IV) chloride indicates that lead has a +4 oxidation state, while copper(II) oxide indicates copper has a +2 oxidation state. Understanding these names helps in identifying the correct formulas and their corresponding weights.
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Polyatomic Ions
Polyatomic ions are charged entities composed of two or more atoms covalently bonded, which function as a single ion. Examples include the perchlorate ion (ClO4-) in sodium perchlorate (NaClO4) and the iodate ion (IO3-) in iodic acid (HIO3). Recognizing these ions is crucial for correctly writing formulas and calculating their weights, as they often dictate the overall charge and composition of the compound.
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Related Practice
Textbook Question
Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (b) NH4NO3(s) → N2O(g) + H2O(g) (c) Zn(OH)2(s) → ZnO(s) + H2O(l) (d) Ag2O(s) → Ag(s) + O2(g)
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Textbook Question
Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) C3H6(s) + O2(g) → CO2(g) + H2O(l)
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Textbook Question
Determine the formula weights of each of the following compounds: (a) Butyric acid, CH3CH2CH2COOH, which is responsible for the rotten smell of spoiled food (b) sodium perborate, NaBO3, a substance used as bleach (c) CF2Cl2, a refrigerant known as Freon (d) NaHCO3, known as baking soda and used in bread and pastry baking (e) isopentyl acetate, CH3CO2C5H11, responsible for the odor of bananas.
Textbook Question
Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) NaClO3(s) → NaCl(s) + O2(g) (b) NH4OH(aq) → H2O(l) + NH3(g) (c) K(s) + Cl2(g) → KCl(s) (d) C2H5OH(l) + O2(g) → CO2(g) + H2O(l)
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Textbook Question
Calculate the percentage by mass of oxygen in the following compounds: (a) vanillin, C8H8O3