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Show how Equations 18.7 and 18.9 can be added to give Equation 18.10.
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Ch.18 - Chemistry of the Environment
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
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 18, Problema 62
Suppose that on another planet the atmosphere consists of 17% Kr, 38% CH4, and 45% O2. What is the average molar mass at the surface? What is the average molar mass at an altitude at which all the O2 is photodissociated?
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Identify the components of the atmosphere and their respective percentages: Krypton (Kr) 17%, Methane (CH4) 38%, and Oxygen (O2) 45%.
Calculate the molar mass of each component: Kr = 83.80 g/mol, CH4 = 16.04 g/mol, O2 = 32.00 g/mol.
Determine the average molar mass at the surface using the formula: \( M_{avg} = (\text{fraction of Kr} \times M_{Kr}) + (\text{fraction of CH4} \times M_{CH4}) + (\text{fraction of O2} \times M_{O2}) \).
Consider the scenario at altitude where all O2 is photodissociated, meaning O2 is no longer present. Recalculate the average molar mass using only Kr and CH4: \( M_{avg, altitude} = (\text{fraction of Kr} \times M_{Kr}) + (\text{fraction of CH4} \times M_{CH4}) \).
Adjust the fractions of Kr and CH4 to account for the absence of O2, ensuring their sum equals 100% before recalculating the average molar mass.
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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 molecule. Understanding molar mass is essential for converting between grams and moles, which is crucial for stoichiometric calculations in chemistry.
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02:11
Molar Mass Concept
Average Molar Mass of a Mixture
The average molar mass of a gas mixture is determined by taking the weighted average of the molar masses of the individual components, based on their mole fractions. This concept is important for calculating properties of gas mixtures, such as density and partial pressures, and is essential for solving problems involving atmospheric compositions.
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02:11Molar Mass Concept
Photodissociation
Photodissociation is the process by which a chemical compound is broken down into its constituent atoms or simpler molecules through the absorption of light energy. In the context of the question, understanding photodissociation is crucial for determining how the composition of the atmosphere changes with altitude, particularly the removal of O2 and its impact on the average molar mass.