Domanda del libro di testo
Vanillin, the dominant flavoring in vanilla, contains C, H, and O. When 1.05 g of this substance is completely combusted, 2.43 g of CO2 and 0.50 g of H2O are produced. What is the empirical formula of vanillin?
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- 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
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Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 96
Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 96Capitolo 3, Problema 96
An organic compound was found to contain only C, H, and Cl. When a 1.50-g sample of the compound was completely combusted in air, 3.52 g of CO2 was formed. In a separate experiment, the chlorine in a 1.00-g sample of the compound was converted to 1.27 g of AgCl. Determine the empirical formula of the compound.
Guida verificata passo dopo passo1
Calculate the moles of CO2 produced using its molar mass.
Determine the moles of carbon in the sample from the moles of CO2, since each mole of CO2 contains one mole of carbon.
Calculate the mass of carbon in the sample using the moles of carbon and the atomic mass of carbon.
Determine the moles of AgCl produced using its molar mass, and then find the moles of chlorine in the sample, since each mole of AgCl contains one mole of chlorine.
Calculate the mass of chlorine in the sample using the moles of chlorine and the atomic mass of chlorine, then find the mass of hydrogen by subtracting the masses of carbon and chlorine from the total mass of the sample.
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Combustion Analysis
Combustion analysis is a technique used to determine the composition of organic compounds by burning them in excess oxygen. The products of combustion, typically carbon dioxide (CO2) and water (H2O), are measured to calculate the amounts of carbon and hydrogen in the original sample. In this question, the mass of CO2 produced allows us to infer the amount of carbon in the compound.
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Percorso guidato
01:29
Combustion of Non-Hydrocarbons
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on the conservation of mass. It allows chemists to relate the quantities of substances involved in a reaction. In this case, stoichiometric relationships help convert the mass of CO2 produced into moles of carbon, which is essential for determining the empirical formula of the compound.
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Percorso guidato
01:16Stoichiometry Concept
Empirical Formula
The empirical formula of a compound represents the simplest whole-number ratio of the elements present. It is derived from the amounts of each element calculated from experimental data. In this problem, the empirical formula is determined by finding the moles of carbon, hydrogen, and chlorine in the compound and expressing their ratios in the simplest form.
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02:26Empirical vs Molecular Formula
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A method used by the U.S. Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the air sample through a 'bubbler' containing sodium iodide, which removes the ozone according to the following equation: O31g2 + 2 NaI1aq2 + H2O1l2¡ O21g2 + I21s2 + 2 NaOH1aq2 (a) How many moles of sodium iodide are needed to remove 5.95 * 10-6 mol of O3?
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