Name: gas pressure patterns in kinetic molecular theory
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 34 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.3

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Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

보일, 샤를, 게이 뤼삭, 아보가드로가 유도한 다양한 기체 법칙에 의해 표현된 서로 다른 기체 성질에 대한 관찰은 개념적으로 기체 분자 운동론에 따릅니다. 기체에 의해 가해지는 압력은 끊임없이 운동하는 입자가 용기의 벽에 가하는 충격에서 비롯됩니다. 몰 수와 온도를 일정하게 유지하면서 용기의 부피를 줄이면 기체 입자들이 서로 더 가까워져 입자간의 간격이 줄어듭니다.

부피가 줄어들면 기체의 밀도와 충돌 빈도, 즉 분자와 벽의 충돌 빈도가 증가합니다. 따라서 기체가 가하는 압력이 증가합니다. 압력과 부피 사이의 반비례 관계는 보일의 법칙에 의해 설명됩니다.

일정한 온도에서 용기에 더 많은 몰의 기체를 추가하면 기체의 밀도가 증가하므로 충돌 빈도가 증가합니다. 초기 압력을 유지하려면 부피를 확장해야 합니다. 부피와 몰 사이의 이러한 비례 관계는 아보가드로의 법칙에 의해 설명됩니다.

이제 몰 수는 일정하게 유지되고 온도가 상승하는 경우를 고려해 봅시다. 기체 입자의 평균 운동에너지는 온도에 비례하여 증가하기 때문에 입자들은 더 자주 그리고 더 강하게 충돌합니다. 온도가 상승하는 동안 부피를 일정하게 유지하면 기체의 밀도와 충돌 빈도가 증가하므로 압력도 증가합니다.

압력과 온도 사이의 비례 관계는 게이 뤼삭의 법칙에 의해 설명됩니다. 반면 몰 수가 일정한 조건에서 압력이 일정하게 유지되어야 하는 경우에는 온도 상승과 함께 부피를 증가하여 충돌이 더 큰 표면적으로 확산되도록 해야 합니다. 부피와 온도 사이의 비례 관계는 샤를의 법칙에 의해 설명됩니다.

마지막으로 기체 분자 운동론에 따르면 기체 입자는 서로 밀거나 당기지 않습니다. 서로 다른 기체들의 혼합물에서 구성 분자들은 독립적으로 행동하며 개별적인 압력은 다른 기체의 존재에 의한 영향을 받지 않습니다. 따라서 혼합물의 총 압력은 개별적인 기체 압력의 합입니다.

이것이 돌턴의 법칙입니다.

운동 분자 이론과 가스 법칙은 가스 분자의 특성을 설명합니다.

KMT(운동 분자 이론)와 그 가정의 테스트는 가스의 거동을 설명하고 기술하는 능력입니다. 다양한 기체 법칙(Boyle의 법칙, Charles의 법칙, Gay-Lussac의 법칙, Avogadro의 법칙, Dalton의 법칙)은 KMT의 가정에서 파생될 수 있으며, 이로 인해 화학자들은 이론의 가정이 기체 분자의 특성을 정확하게 나타낸다고 믿게 되었습니다.

운동 분자 이론은 가스의 거동을 설명합니다

가스 압력은 빠르게 움직이는 가스 분자에 의해 가해지고 단위 시간당 벽의 단위 면적에 부딪히는 분자 수에 직접적으로 의존한다는 점을 상기하면서 KMT는 개념적으로 가스의 거동을 다음과 같이 설명합니다.

<ol style="list-style-type: disc;">
	<li>게이뤼삭의 법칙: 온도가 증가하면 기체 분자의 평균 속도와 운동 에너지가 증가합니다. 부피가 일정하게 유지되면 가스 분자의 속도가 증가하여 용기 벽과 더 빈번하고 더 강력한 충돌이 발생하여 압력이 증가합니다. 이를 아몬톤의 법칙이라고도 합니다.</li>
	<li>샤를의 법칙: 기체의 온도가 증가하면 기체가 차지하는 부피가 증가해야만 일정한 압력이 유지될 수 있습니다. 이로 인해 분자가 용기 벽에 도달하기 위해 이동하는 평균 거리가 더 길어지고 벽 표면적이 증가합니다. 이러한 조건은 분자벽 충돌 빈도와 단위 면적당 충돌 횟수를 모두 감소시키며, 그 결합 효과는 더 높은 온도에서 더 큰 운동 에너지로 인해 증가된 충돌력의 효과와 균형을 이룹니다.</li>
	<li>보일의 법칙: 기체 부피가 감소하면 용기 벽 면적이 감소하고 분자벽 충돌 빈도가 증가하여 기체에 의해 가해지는 압력이 증가합니다.</li>
	<li>아보가드로의 법칙: 일정한 압력과 온도에서 분자벽 충돌의 빈도와 힘은 일정합니다. 이러한 조건에서 기체 분자의 수를 늘리려면 증가된 충돌 빈도를 보상하기 위해 단위 면적당 충돌 횟수를 줄이기 위해 용기 부피의 비례적인 증가가 필요합니다.</li>
	<li>돌턴의 법칙: 두 가스 사이의 거리가 멀기 때문에 혼합물에 있는 한 가스의 분자는 다른 가스가 있든 없든 동일한 주파수로 용기 벽에 충격을 가하며, 가스 혼합물의 총 압력은 다음의 합과 같습니다. 개별 가스의 부분) 압력.</li>
</ol>

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/9-5-the-kinetic-molecular-theory">Openstax, Chemistry 2e, Section 9.5: The Kinetic-Molecular Theory.</a>

운동 분자 이론(KMT)과 그 가정의 테스트는 기체의 거동을 설명하고 설명하는 능력입니다. 다양한 가스 법칙 ...

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gas pressure patterns in kinetic molecular theory

Kinetic molecular theory explains gas pressure by linking it to the motion of gas molecules. Gas pressure comes from rapidly moving molecules hitting the walls of a container. It depends on how many molecules strike a unit area in a given time.

The theory also helps explain the main gas laws. In Gay-Lussac’s law, also called Amontons’s law, raising temperature increases the average speed and kinetic energy of gas molecules. If volume stays constant, the molecules collide with the walls more often and more forcefully, so pressure increases.

Charles’s law shows what happens when temperature rises at constant pressure. The gas must expand to keep pressure steady. That larger volume means molecules travel farther before reaching the walls, and the wall area increases too. These changes lower collision frequency and the number of collisions per unit area, which balances the stronger collisions caused by the higher kinetic energy.

Boyle’s law describes the effect of smaller volume. When gas volume decreases, the container wall area also decreases. Molecule-wall collisions become more frequent, and the pressure rises. Avogadro’s law says that at constant pressure and temperature, the collision rate and collision force stay constant. If the number of gas molecules increases, the volume must increase in proportion so the collisions per unit area can drop enough to offset the added molecules.

Dalton’s law applies to gas mixtures. Because gas molecules are far apart, one gas in a mixture strikes the container walls with the same frequency whether other gases are present or not. The total pressure of the mixture equals the sum of the partial pressures of the individual gases. These gas laws show how the assumptions of kinetic molecular theory fit the behavior of gases.

Gas Pressure Patterns in Kinetic Molecular Theory

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definition and measurement of pressure: atmospheric pressure, barometer, and manometer

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Pressure Units and Tools for Gas Measurement

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Gas pressure, volume, temperature, and amount are linked by several gas laws. Scientists found these relationships by studying how a confined gas changes when one variable is held constant and another changes. These patterns apply to an ideal gas, which is a useful model for gases under low pressure and high temperature. Gay-Lussac’s law, also called Amontons’s law, connects pressure and temperature. If gas is trapped in a rigid container, the volume and number of moles stay constant. When the...

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Gas Pressure in Mixtures: Partial Pressures

Gas pressure in mixtures is described by partial pressure and mole fraction. When gases do not chemically react, each gas in the mixture acts as if it were alone in the container. The pressure from one gas is called its partial pressure. For a mixture of three gases, A, B, and C, the total pressure equals the sum of their partial pressures: PA, PB, and PC. This is Dalton's law of partial pressures. It states that the total pressure of a mixture of ideal gases is the sum of the pressures from...

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basic postulates of kinetic molecular theory: particle size, energy, and collision

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Kinetic molecular theory explains gas behavior at the particle level. It gives a microscopic model for what happens when pressure or temperature changes. Gas laws describe how macroscopic properties change, but they do not explain why those changes happen. The theory was put into a complete form by Rudolf Clausius in 1857. It was built from hundreds of experimental observations about gases. Those observations helped explain the different gas laws through a few basic postulates. One key idea...

kinetic molecular theory and gas laws explain properties of gas molecules

Kinetic molecular theory explains gas pressure by linking it to the motion of gas molecules. Gas pressure comes from rapidly moving molecules hitting the walls of a container. It depends on how many molecules strike a unit area in a given time. The theory also helps explain the main gas laws. In Gay-Lussac’s law, also called Amontons’s law, raising temperature increases the average speed and kinetic energy of gas molecules. If volume stays constant, the molecules collide with the walls more...

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key terms and concepts

Explore how kinetic molecular theory explains gas pressure, temperature, volume changes, and the gas laws of Boyle, Charles, Gay-Lussac, Avogadro, and Dalton.

Gas Pressure Patterns in Kinetic Molecular Theory | JoVE K12

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Phase Transitions: Melting and Freezing

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Phase Diagrams

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First Law of Thermodynamics

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Internal Energy

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Quantifying Heat

Thermal Energy&#160;

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Quantifying Work

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Enthalpy

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Thermochemical Equations

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Constant Pressure Calorimetry

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Constant Volume Calorimetry

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Standard Enthalpy of Formation

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PS.Chm.7.2

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Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

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Gas Pressure Patterns in Kinetic Molecular Theory

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