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

ضع في اعتبارك غاز أكسجين في حاوية كتلتها المولية 0.0320 كجم/مول في درجة حرارة الغرفة. حدد نسبة عدد الجزيئات التي تبلغ سرعتها حوالي 400 م / ث إلى عدد الجزيئات التي تبلغ سرعتها حوالي 200 م / ث ، وسرعة الجذر ومتوسط التربيع ، والسرعة الأكثر احتمالا لجزيئات الأكسجين في درجة حرارة الغرفة.
لحل المشكلة ، حدد الكميات المعروفة وغير المعروفة.
في الشكل التفاضلي ، يكون عدد الجزيئات القريبة من السرعة هو نتاج دالة التوزيع الاحتمالي للسرعة مضروبا في فاصل صغير من السرعة.
يمكن حساب النسبة بقسمة عدد الجزيئات القريبة من السرعات الفردية.
استبدل المصطلحات الموجودة في دالة توزيع ماكسويل بولتزمان بجزيئات الغاز. يمكن تحديد نسبة عدد الجزيئات ذات السرعات الفردية.
تذكر معادلة السرعة الجذر ومتوسط التربيع ومعادلة السرعة الأكثر احتمالا لجزيئات الغاز. من خلال استبدال القيم المعروفة ، يمكن تحديد سرعة الجذر ومتوسط التربيع والسرعة الأكثر احتمالا للغاز.

<ol>
	<li>OpenStax. (2019). جامعة الفيزياء المجلد 2. [نسخة الويب] ، الصفحات 94-95. تم الاسترجاع من <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>

توزيع ماكسويل بولتزمان: حل المشكلات

<div style="direction:rtl">تتحرك الجزيئات الفردية في الغاز في اتجاهات عشوائية، لكن الغاز الذي يحتوي على العديد من الجزيئات له توزيع يمكن التنبؤ به للسرعات الجزيئية، وهو ما يعرف بتوزيع ماكسويل-بولتزمان، f(v). 

يتم تعريف دالة التوزيع f(v) بالقول أن الرقم المتوقع N (v1,v2) من الجسيمات بسرعات تتراوح بين v1 و v2 يتم تقديمها بواسطة


<img alt="Equation1" src="/files/ftp_upload/14167/14167_Equation_1.svg" style="text-align: center; height: 80px;"> 

بما أن N ليس له أبعاد ووحدة f(v) هي ثانية لكل متر، فيمكن أن تكون المعادلة ملائمة تم تعديله إلى شكل تفاضلي:

<img alt="Equation2" src="/files/ftp_upload/14167/14167_Equation_2.svg" style="text-align: center; height: 20px;"> 

ضع في اعتبارك عينة من غاز النيتروجين في أسطوانة كتلتها المولية 28.0 جم/مول عند درجة حرارة الغرفة 27 درجة مئوية. حدد نسبة عدد الجزيئات ذات السرعة المتجهة المتجهة المتجهة المتجهة القريبة جدًا من 300 م/ث إلى عدد الجزيئات ذات السرعة المتجهة المتجهة المتجهة المتجهة القريبة جدًا من 100 م/ث. 

لحل المشكلة قم بدراسة الموضع وتحديد الكميات المعروفة وغير المعروفة. ثانيًا، قم بتحويل كافة القيم المعروفة إلى وحدات النظام الدولي المناسبة. على سبيل المثال، قم بتحويل الوزن الجزيئي إلى كيلوجرام (kg) ودرجة الحرارة إلى كلفن (K). تذكر دالة التوزيع لمعادلة السرعة المتجهة المتجهة. وأخيرًا، عوض بالقيم المعلومة في المعادلة لتحديد الكمية المجهولة. 

<img alt="Equation3" src="/files/ftp_upload/14167/14167_Equation_3.svg" style="text-align: center; height: 280px;"></div>

تتحرك الجزيئات الفردية في الغاز في اتجاهات عشوائية ، لكن الغاز الذي يحتوي على العديد من الجزيئات له توزيع يمكن التنبؤ به للسرعات الجزيئية ، والتي ...

Education

JoVE Core

Physics

الفيزياء

Unit 1

الوحدة الأولى

The Kinetic Theory of Gases

النظرية الحركية للغازات

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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

The ideal gas equation links pressure, volume, temperature, and amount of gas. It describes a hypothetical gas and is built from four empirical gas laws: Boyle’s law, Charles’s law, Avogadro’s law, and Gay-Lussac’s law. When these proportionalities are combined, they give one constant called the universal gas constant. This gas constant has the same value for all real gases under certain conditions. In chemical calculations, that constant is used in the ideal gas equation. The equation works...

van der waals equation

How Real Gases Deviate from Ideal Behavior

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pv-diagrams

Liquid-Gas Changes on pV Curves

pV curves show how gas pressure changes with volume. A pV diagram is a graph of pressure versus volume for the gas being studied. It helps describe how the substance behaves. When the gas acts like an ideal gas, the ideal gas equation gives the link between pressure and volume. A common pV curve is an isotherm, which is a line drawn at fixed temperature and fixed number of molecules. For an ideal gas, pressure times volume stays constant. That means volume goes down as pressure goes up. The...

kinetic theory of an ideal gas

Avogadro's Number and Gas Particle Motion

Avogadro's number and gas particle motion help explain how gases behave at the particle level. A mole is the amount of a substance that contains as many molecules as there are atoms in exactly 12 grams of carbon-12. This idea came from Amedeo Avogadro, who proposed that equal volumes of gas at the same pressure and temperature contain equal numbers of molecules, no matter what the gas is. Avogadro's number is the number of molecules in one mole. Its value is 6.02 × 10^23 mol−1. This number...

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

physics

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Maxwell-Boltzmann Gas Speed Ratio

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