Domanda del libro di testo
Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) number of molecules?
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Ch.10 - Gases
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 10, Problema 80c
Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (c) average kinetic energy of the molecules?
Guida verificata passo dopo passo1
Step 1: Understand the concept of kinetic energy. The average kinetic energy of a gas molecule is directly proportional to the temperature of the gas in Kelvin. It is given by the equation KE_avg = 3/2 kT, where k is Boltzmann's constant and T is the temperature in Kelvin.
Step 2: Recall that STP (Standard Temperature and Pressure) refers to a temperature of 273.15 K and a pressure of 1 atm. Therefore, both the N2 and CH4 gases are at the same temperature.
Step 3: Since the average kinetic energy of a gas molecule is directly proportional to the temperature, and both gases are at the same temperature, they will have the same average kinetic energy.
Step 4: Note that the type of gas (N2 or CH4 in this case) does not affect the average kinetic energy of the molecules. The average kinetic energy of the molecules in a gas only depends on the temperature.
Step 5: Therefore, the average kinetic energy of the molecules in the N2 and CH4 gases are the same at STP.
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Kinetic Molecular Theory
The Kinetic Molecular Theory explains the behavior of gases in terms of particle motion. It states that gas molecules are in constant, random motion and that the average kinetic energy of these molecules is directly proportional to the temperature of the gas in Kelvin. This theory helps us understand how temperature influences the speed and energy of gas particles.
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01:19
Kinetic Molecular Theory
Average Kinetic Energy
The average kinetic energy of gas molecules can be calculated using the formula KE = (3/2)kT, where k is the Boltzmann constant and T is the absolute temperature in Kelvin. At standard temperature and pressure (STP), both N2 and CH4 are at the same temperature, meaning their average kinetic energies will be equal, regardless of their molecular weights.
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00:34Kinetic & Potential Energy
Molecular Mass and Speed
While the average kinetic energy of gas molecules at the same temperature is the same, the speed of the molecules varies with their mass. Lighter molecules, like CH4, move faster than heavier molecules, like N2, at the same temperature. This difference in speed can affect the rate of diffusion and other properties, but does not change the average kinetic energy at STP.
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00:57Speed of Light Formula
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