교과서 질문
Consider the following gases, all at STP: Ne, SF6, N2, CH4. (d) Which one has the highest total molecular volume relative to the space occupied by the gas?
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Ch.10 - Gases
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
10장, 문제 113f
Consider the following gases, all at STP: Ne, SF6, N2, CH4. (f) Which one would effuse more rapidly than N2?
검증된 단계별 안내1
Identify the concept of effusion and relate it to Graham's law, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.
List the molar masses of the given gases: Ne (Neon), SF_6 (Sulfur hexafluoride), N_2 (Nitrogen), and CH_4 (Methane).
Calculate the molar mass of each gas: Ne = 20.18 g/mol, SF_6 = 146.06 g/mol, N_2 = 28.02 g/mol, CH_4 = 16.04 g/mol.
Compare the molar masses of the gases to that of N_2. According to Graham's law, a gas with a lower molar mass than N_2 will effuse more rapidly.
Determine which gas has a molar mass less than that of N_2 and conclude that this gas will effuse more rapidly than N_2.
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1m주요 개념
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Graham's Law of Effusion
Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases effuse more quickly than heavier gases. For example, if comparing nitrogen (N2) with other gases, the gas with a lower molar mass than nitrogen will effuse more rapidly.
추천 영상:
가이드 코스
2:03
Graham's Law of Effusion
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is a critical factor in determining the rate of effusion according to Graham's Law. In this context, knowing the molar masses of Ne, SF6, N2, and CH4 allows us to predict which gas will effuse faster than nitrogen.
추천 영상:
가이드 코스
02:11Molar Mass Concept
Standard Temperature and Pressure (STP)
Standard Temperature and Pressure (STP) is defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (atm). At STP, the behavior of gases can be compared more easily, as their properties are standardized. This context is essential for analyzing the effusion rates of the gases mentioned in the question.
추천 영상:
가이드 코스
01:08Standard Temperature and Pressure
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교과서 질문
Consider the following gases, all at STP: Ne, SF6, N2, CH4. (g) Which one would have the largest van der Waals b parameter?
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교과서 질문
Consider the following gases, all at STP: Ne, SF6, N2, CH4. (a) Which gas is most likely to depart from the assumption of the kinetic-molecular theory that says there are no attractive or repulsive forces between molecules?
1083
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