Name: maxwell-boltzmann gas speed ratio
Uploaded: 2023-09-18T17:11:17.000Z
Duration: 1 min 20 s
Channel: JoVE

K12 Standards

Florida Department of Education

High School

Physical Science

SC.912.P.12

SC.912.P.12.10

maxwell-boltzmann-distribution-problem-solving

Maxwell-Boltzmann Distribution: Problem Solving

Rozważmy gazowy tlen w pojemniku o masie molowej 0,0320 kg/mol w temperaturze pokojowej. Określ stosunek liczby cząsteczek o prędkości około 400 m/s do liczby cząsteczek o prędkości około 200 m/s, prędkości średniej kwadratowej i najbardziej prawdopodobnej prędkości cząsteczek tlenu w temperaturze pokojowej.
Aby rozwiązać problem, zidentyfikuj znane i nieznane ilości.
W postaci różniczkowej liczba cząsteczek bliskich prędkości jest iloczynem funkcji rozkładu prawdopodobieństwa prędkości pomnożonej przez mały przedział prędkości.
Stosunek ten można obliczyć, dzieląc liczbę cząsteczek w pobliżu poszczególnych prędkości.
Zastąp cząsteczki gazu składnikami funkcji rozkładu Maxwella-Boltzmanna. Można określić stosunek liczby cząsteczek do poszczególnych prędkości.
Przypomnij sobie równanie prędkości średniej kwadratowej i najbardziej prawdopodobne równanie prędkości dla cząsteczek gazu. Podstawiając znane wartości, można określić średnią kwadratową prędkości i najbardziej prawdopodobną prędkość gazu.

<ol>
	<li>Protokół OpenStax. (2019). Fizyka uniwersytecka Vol. 2. [Wersja internetowa], strony 94–95. Źródło: <a href="https://openstax.org/books/university-physics-volume-2/pages/2-4-distribution-of-molecular-speeds">https://openstax.org/books/university-physics-volume-2/pages/2-4-distribution-of-molecular-speeds</a></li>
</ol>

rozkład maxwella-boltzmanna: rozwiązywanie problemów

Poszczególne cząsteczki w gazie poruszają się w przypadkowych kierunkach, ale gaz zawierający wiele cząsteczek ma przewidywalny rozkład prędkości molekularnych, znany jako rozkład Maxwella-Boltzmanna, f(v ).

Ta funkcja rozkładu f(v) jest zdefiniowana w ten sposób, że oczekiwana liczba N (v1,v2) cząstek o prędkościach od v1 i v2 ─ są podawane przez

<img alt="Równanie1" src="/files/ftp_upload/14167/14167_Equation_1.svg" style="text-align: center; height: 80px;" />

Ponieważ N jest bezwymiarowe, a jednostką f(v) jest sekunda na metr, równanie można wygodnie zapisać zmodyfikowany do postaci różniczkowej:

<img alt="Równanie2" src="/files/ftp_upload/14167/14167_Equation_2.svg" style="text-align: center; height: 20px;" />

Rozważ próbkę gazowego azotu w cylindrze o masie molowej 28,0 g/mol w temperaturze pokojowej 27 °C. Określ stosunek liczby cząsteczek poruszających się z prędkością bardzo bliską 300 m/s do liczby cząsteczek poruszających się z prędkością bardzo bliską 100 m/s.

Aby rozwiązać problem, zbadaj sytuację i zidentyfikuj znane i nieznane wielkości.

Po drugie, przelicz wszystkie znane wartości na odpowiednie jednostki SI. Na przykład przelicz masę cząsteczkową na kilogramy (kg), a temperaturę na kelwiny (K). Przypomnijmy sobie rozkład rozkładu równania prędkości. Na koniec podstaw znane wartości do równania, aby określić nieznaną wielkość.

<img alt="Równanie3" src="/files/ftp_upload/14167/14167_Equation_3.svg" style="text-align: center; height: 280px;" />

Rozkład Maxwella-Boltzmanna: rozwiązywanie problemów

Poszczególne cząsteczki w gazie poruszają się w losowych kierunkach, ale gaz zawierający wiele cząsteczek ma przewidywalny rozkład prędkości molekularnych, który ...

Education

JoVE Core

Physics

Fizyka

Unit 1

Jednostka 1

The Kinetic Theory of Gases

Kinetyczna teoria gazów

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

maxwell-boltzmann gas speed ratio

The Maxwell-Boltzmann distribution describes how molecular speeds are spread in a gas. Even though individual molecules move in random directions, the whole gas has a predictable speed pattern. This distribution is written as f(v), where v is molecular speed.

The distribution function is used to find the expected number of particles with speeds between v1 and v2. Because N is dimensionless, f(v) has units of seconds per meter. The relationship can also be written in differential form for speed intervals that are very small.

A nitrogen gas sample in a cylinder gives a sample problem. The gas has a molar mass of 28.0 g/mol and a room temperature of 27 °C. The task is to find the ratio of molecules with speeds very close to 300 m/s to those with speeds very close to 100 m/s.

Solving the problem starts with identifying the known and unknown quantities. The next step is to convert the given values into SI units. That means changing the molar mass to kilograms and the temperature to kelvin. After that, the Maxwell-Boltzmann velocity equation is used, and the known values are substituted to calculate the ratio.

Maxwell-Boltzmann Gas Speed Ratio

equation of state

Gas Behavior in the Equation of State

The equation of state describes how a gas’s pressure, volume, temperature, and number of moles are related. These macroscopic properties help define the condition, or state, of the matter in a thermodynamics system. The relationship between these quantities can be written as a simple mathematical expression. In some cases, it is too complex to express in a formula. Even then, the link between the quantities still exists. When an equation of state cannot be written mathematically, scientists...

ideal gas equation

Gas Laws Behind the Ideal Equation

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van der waals equation

How Real Gases Deviate from Ideal Behavior

Real gases often deviate from the ideal gas law, especially at low temperatures and high pressures. The van der Waals equation improves the ideal gas model by adding two corrections that account for these real-world effects. One correction accounts for attractive forces between molecules. These forces become stronger at higher densities and lower the measured pressure, so the equation adds a pressure term based on the square of the molar density and a positive constant a. The second...

pv-diagrams

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kinetic theory of an ideal gas

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molecular kinetic energy

Gas Pressure and Molecular Motion

Gas pressure comes from the motion of molecules in a container. The word gas came from a Flemish word meaning “chaos,” and J. B. van Helmont first used it to describe vapors. In a gas, molecules move in a continuous and random way. When a molecule hits a container wall, its velocity changes. The part of the velocity parallel to the wall stays the same. The part perpendicular to the wall reverses direction, but its size does not change. If the molecule’s velocity changes in the x-direction, its...

distribution of molecular speeds

Molecular Speed Curves and Vapor Pressure

Molecular speed curves show how the speeds of gas particles are spread out at a given temperature. For a gas with many molecules, this spread is predictable even though each molecule moves randomly in direction and speed. The pattern is called the Maxwell-Boltzmann distribution. Liquids have a similar speed distribution, but it is not exactly the same as in gases. This difference helps explain boiling and vapor pressure. A molecule must reach at least a certain speed, v a, to escape from the...

maxwell-boltzmann distribution: problem solving

The Maxwell-Boltzmann distribution describes how molecular speeds are spread in a gas. Even though individual molecules move in random directions, the whole gas has a predictable speed pattern. This distribution is written as f(v), where v is molecular speed. The distribution function is used to find the expected number of particles with speeds between v1 and v2. Because N is dimensionless, f(v) has units of seconds per meter. The relationship can also be written in differential form for speed...

phase diagram

Water Phase Changes on a Pressure Chart

Water phase changes can be mapped on a pressure and temperature chart called a phase diagram. These plots show which phase a substance is in at different conditions. They also reveal where phase transitions happen, because the boundary lines mark the temperatures and pressures where two phases coexist. The water phase diagram shows how pressure affects boiling. As pressure rises, the boiling temperature increases gradually until it reaches 374 °C at 218 atm. A pressure cooker works this way.

mean free path and mean free time

Gas collisions: path length and time

Gas collisions in a cylinder help explain the mean free path and mean free time. Gas molecules move in random motion. They collide with each other and change speed and direction. The mean free path is the average path length between collisions. The mean free path depends on how many molecules are packed into a volume. It varies inversely with density. When more molecules are present, collisions happen more often, so the mean free path becomes shorter. It also depends on molecule size. Larger...

heat capacity: problem-solving

Heat Capacity of Gases by Degrees of Freedom

Heat capacity of gases depends on the gas type and the motion of its molecules. It is the amount of heat energy needed to raise the temperature of a unit mass of gas by one degree Celsius. This thermodynamic property is important in science and industry. To solve heat capacity problems, first identify the gas. A gas's molecular structure affects its heat capacity because the molecules have different degrees of freedom. These values can be found from tables or from empirical equations. Next,...

dalton's law of partial pressure

Gas Mixtures and Their Partial Pressures

Gas mixtures have a total pressure that comes from the partial pressures of each gas. A partial pressure is the pressure one gas would make if it filled the whole container by itself. This idea helps explain how gases behave when they are mixed together. When two or more gases share a container, their molecules move randomly and collide with one another. If the gases are at the same temperature, they reach thermal equilibrium. Their molecules then have the same average kinetic energy. In that...

escape velocities of gases

Why Lighter Gases Escape Earth First

Earth’s escape velocity is the speed an object needs to leave gravity behind. Near the top of the atmosphere, about 100 km above Earth, that speed is 11.1 km/s. Gas molecules can escape only if their speeds become high enough to reach that limit. The chance of escape depends on gas temperature and molecular speed. According to kinetic theory, the average kinetic energy of gas molecules is proportional to temperature. As temperature rises, the rms speed, or root-mean-square speed, also rises.

key terms and concepts

Solve a Maxwell-Boltzmann distribution problem for nitrogen gas by converting units, using the velocity equation, and comparing molecule speed ratios.

Maxwell-Boltzmann Gas Speed Ratio | JoVE K12

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Maxwell-Boltzmann Gas Speed Ratio

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