Domanda del libro di testo
Write the structural formulas of three different compounds that each have the molecular formula C5H12.
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Ch.3 - Molecules and Compounds
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 3, Problema 135
Find the total number of atoms in a sample of cocaine hydrochloride, C17H22ClNO4, of mass 23.5 mg.
Guida verificata passo dopo passo1
Convert the mass of the cocaine hydrochloride from milligrams to grams. Remember that 1 mg equals 0.001 grams.
Calculate the molar mass of cocaine hydrochloride, C17H22ClNO4. Use the atomic masses of carbon (C), hydrogen (H), chlorine (Cl), nitrogen (N), and oxygen (O) from the periodic table to find the sum.
Use the molar mass to convert the mass of the cocaine hydrochloride sample from grams to moles. Use the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}} \).
Calculate the total number of molecules in the sample by using Avogadro's number, which is approximately \(6.022 \times 10^{23}\) molecules per mole. Multiply the number of moles by Avogadro's number.
Determine the total number of atoms in a molecule of cocaine hydrochloride. Since the formula is C17H22ClNO4, add up the atoms: 17 carbon atoms, 22 hydrogen atoms, 1 chlorine atom, 1 nitrogen atom, and 4 oxygen atoms. Multiply the total number of molecules by the total number of atoms per molecule to find the total number of atoms in the sample.
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Molecular Formula
The molecular formula of a compound provides the types and numbers of atoms present in a molecule. For cocaine hydrochloride, C17H22ClNO4, the formula indicates it contains 17 carbon (C) atoms, 22 hydrogen (H) atoms, 1 chlorine (Cl) atom, 1 nitrogen (N) atom, and 4 oxygen (O) atoms. Understanding the molecular formula is essential for determining the total number of atoms in a given mass of the substance.
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02:08
Determining Molecular Formulas
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the total number of atoms in a sample, one must first calculate the molar mass of cocaine hydrochloride by summing the atomic masses of all atoms in its molecular formula. This value allows for the conversion of the sample's mass into moles, which is crucial for further calculations.
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02:11Molar Mass Concept
Avogadro's Number
Avogadro's number, approximately 6.022 x 10^23, is the number of particles (atoms, molecules, etc.) in one mole of a substance. Once the number of moles of cocaine hydrochloride is determined from the sample's mass and its molar mass, Avogadro's number can be used to calculate the total number of individual atoms in the sample. This concept is fundamental in bridging the macroscopic and microscopic worlds in chemistry.
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02:11Avogadro's Law
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A hydrate of copper(II) chloride has the following formula: CuCl2 • x H2O. The water in a 3.41-g sample of the hydrate is driven off by heating. The remaining sample has a mass of 2.69 g. Find the number of waters of hydration (x) in the hydrate.
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Researchers obtained the following data from experiments to find the molecular formula of benzocaine, a local anesthetic, which contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 3.54-g sample of benzocaine with excess O2 forms 8.49 g of CO2 and 2.14 g H2O. Another 2.35-g sample contains 0.199 g of N. The molar mass of benzocaine is 165 g/mol. Find the molar formula of benzocaine.
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