Ch.22 - Chemistry of the Nonmetals
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
22장, 문제 84
Complete the exercises below. A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of H₂SO₄ consists of three main chemical processes: a. oxidation of S to SO₂, b. oxidation of SO₂ to SO₃, c. the dissolving of SO₃ in H₂SO₄ and the subsequent reaction with water to form H₂SO₄. If the third process produces 130 kJ/mol, how much heat is produced in preparing a mole of H₂SO₄ from a mole of S? How much heat is produced in preparing 5000 pounds of H₂SO₄?
검증된 단계별 안내1
Step 1: Identify the chemical reactions involved in the synthesis of H₂SO₄. The reactions are: (a) S + O₂ → SO₂, (b) 2 SO₂ + O₂ → 2 SO₃, (c) SO₃ + H₂O → H₂SO₄.
Step 2: Determine the enthalpy change for each reaction. You are given that the third process produces 130 kJ/mol. You will need to find or be given the enthalpy changes for the first two reactions to calculate the total heat produced.
Step 3: Calculate the total heat produced per mole of H₂SO₄ by summing the enthalpy changes of the three reactions. This will give you the total heat produced when one mole of sulfur is converted to one mole of H₂SO₄.
Step 4: Convert 5000 pounds of H₂SO₄ to moles. Use the molar mass of H₂SO₄ (approximately 98.08 g/mol) and the conversion factor from pounds to grams (1 pound = 453.592 grams) to find the number of moles.
Step 5: Calculate the total heat produced for 5000 pounds of H₂SO₄ by multiplying the number of moles calculated in Step 4 by the total heat produced per mole from Step 3.
주요 개념
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Thermochemistry
Thermochemistry is the study of the heat energy associated with chemical reactions and changes of state. It involves understanding how energy is absorbed or released during chemical processes, which is crucial for calculating the heat produced or consumed in reactions, such as the formation of sulfuric acid from sulfur.
추천 영상:
가이드 코스
01:49
Chemical Bonds
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances involved in reactions, which is essential for determining how much heat is produced when synthesizing sulfuric acid from sulfur.
추천 영상:
가이드 코스
01:16Stoichiometry Concept
Calorimetry
Calorimetry is the measurement of heat transfer during chemical reactions or physical changes. It provides the tools and methods to quantify the heat produced or absorbed, such as the 130 kJ/mol released in the formation of sulfuric acid, enabling calculations for larger quantities like 5000 pounds of H₂SO₄.
추천 영상:
가이드 코스
00:50Constant-Volume Calorimetry
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