Textbook Question
Refer to the nomenclature flowchart (Figure 3.11) to name each compound. a. KClO3 b. I2O5 c. PbSO4
Ch.3 - Molecules, Compounds & Chemical Equations
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Chapter 3, Problem 59a,b,c,d
Calculate the formula mass for each compound. a. NO2 c. C6H12O6 b. C4H10 d. Cr(NO3)3
Verified step by step guidance1
Identify the number of each type of atom in the molecular formula C6H12O6. This compound contains 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms.
Find the atomic mass of each type of atom from the periodic table. Typically, the atomic mass of Carbon (C) is approximately 12.01 amu, Hydrogen (H) is about 1.008 amu, and Oxygen (O) is around 16.00 amu.
Multiply the atomic mass of each atom by the number of atoms of that element in the molecule. For Carbon: 12.01 amu \(\times\) 6, for Hydrogen: 1.008 amu \(\times\) 12, and for Oxygen: 16.00 amu \(\times\) 6.
Add the total masses of each element together to find the total formula mass of the compound. Sum the products from the previous step.
The result from the previous step gives you the formula mass of C6H12O6 in atomic mass units (amu).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass
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 the atoms in a chemical formula. For example, in glucose (C6H12O6), the molar mass is determined by adding the masses of 6 carbon (C), 12 hydrogen (H), and 6 oxygen (O) atoms.
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Molar Mass Concept
Atomic Mass
Atomic mass is the weighted average mass of an element's isotopes, measured in atomic mass units (amu). Each element has a specific atomic mass listed on the periodic table, which is used to calculate the molar mass of compounds. For instance, carbon has an atomic mass of approximately 12.01 amu, hydrogen about 1.01 amu, and oxygen around 16.00 amu.
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Chemical Formula
A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. In the case of glucose (C6H12O6), the formula shows that it contains 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms. Understanding the chemical formula is essential for calculating the formula mass, as it directly informs the quantities of each element involved.
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Related Practice
Textbook Question
Refer to the nomenclature flowchart (Figure 3.11) to name each compound. a. XeO3 b. KClO
Textbook Question
Calculate the formula mass for each compound. a. MgBr2 b. HNO2 c. CBr4 d. Ca(NO3)2
Textbook Question
Refer to the nomenclature flowchart (Figure 3.11) to name each compound. c. CoSO4