Name: kinetic molecular theory and gas behavior
Uploaded: 2020-09-03T13:38:26.000Z
Duration: 2 min 43 s
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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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Basic Postulates of Kinetic Molecular Theory: Particle Size, Energy, and Collision

Gaz yasaları ideal gazların farklı özellikleri arasındaki ilişkileri özetlerken kinetik moleküler teori, gazların neden yasaları takip ettiğini açıklar. Teori birkaç varsayıma veya kabule dayanmaktadır. İlk varsayım, gaz parçacıklarının boyut olarak ihmal edilebilir olmasıdır.Bir gaz, çoğunlukla kendi boyutlarından çok daha büyük mesafelerde ayrılan küçük parçacıklardan oluşan boş bir alandır. Gazın içinde bulunduğu toplam hacme göre birleşik hacimleri ihmal edilebilir düzeydedir. Parçacıklar arası boşlukları birbirine yakın olması nedeniyle sıkıştırılamayan katı ve sıvıların aksine, gazlar yüksek oranda sıkıştırılabilir.Gaz parçacıkları, rastgele yönlerde düz çizgiler boyunca sabit bir hareket halindedir. Yolları yalnızca diğer parçacıklarla veya kaplarının duvarlarıyla çarpıştıklarında değişir. İkinci varsayım, gaz parçacıklarının tamamen esnek çarpışmalar yapmasıdır.Birbirlerine yapışmadan çarpışırlar ve birbirleri üzerinden sekerler. Bu, bir bilardo oyunu sırasında bilardo topları arasındaki çarpışmalara benzetilebilir. Gaz parçacıkları çarpıştığında birbirleriyle enerji alışverişinde bulunurlar, ancak net enerji kaybı olmaz.Diğer bir deyişle, sistemin toplam enerjisi sabit kalır. Gaz parçacıkları sürekli hareket eder, yani kinetik enerjiye sahiptirler. Bu nedenle, üçüncü varsayım, bir gazın ortalama kinetik enerjisinin kelvin cinsinden mutlak sıcaklığıyla orantılı olduğunu ifade eder.Bu, kinetik enerjinin sıcaklıkla arttığı ve dolayısıyla parçacıkların daha hızlı hareket ettiği anlamına gelir. Daha yüksek sıcaklıklarda hızları artar. Tersine, sıcaklık düştükçe parçacıkların kinetik enerjisi azalır ve daha yavaş hareket ederler.Belirli bir sıcaklıkta, moleküler kütlelerine bakılmaksızın tüm gazlar aynı ortalama kinetik enerjiye sahiptir. Kinetik enerji, kütle çarpı hızın karesine eşittir. Bu nedenle, farklı gazların aynı ortalama kinetik enerjiye sahip olması için, gaz parçacıklarının farklı ortalama hızlarda hareket etmesi gerekir.Bu nedenle, daha ağır gazlar daha düşük ortalama hızlara sahipken, daha hafif gazlar daha yüksek ortalama hızlara sahiptir. Örneğin, helyum ve neon aynı sıcaklıktayken aynı ortalama kinetik enerjiye sahiptir. Bununla birlikte, kütlelerindeki farklılık nedeniyle neon atomları helyum atomlarından çok daha yavaş hareket eder.

kinetik moleküler teori: temel varsayımlar

Ampirik olan ideal gaz denklemi, gazların makroskopik özellikleri arasında ilişkiler kurarak davranışlarını tanımlar. Örneğin, Charles yasası hacim ve sıcaklığın doğrudan ilişkili olduğunu belirtir. Bu nedenle gazlar, sabit basınçta ısıtıldığında genişler. Gaz yasaları makroskopik özelliklerin birbirine göre nasıl değiştiğini açıklasa da, bunun altında yatan mantığı açıklamazlar.
 
 Kinetik moleküler teori, basınç veya sıcaklık değişimi gibi koşullar altında moleküler veya atomik seviyedeki gaz parçacıklarına ne olduğunu anlamaya yardımcı olan mikroskobik bir modeldir. 1857'de Rudolf Clausius, gazların davranışının yüzlerce deneysel gözlemine dayanarak geliştirilen varsayımlarla farklı gaz yasalarını etkili bir şekilde açıklayan teorinin eksiksiz ve tatmin edici bir formunu yayınlamıştır.
 
 Bu teorinin göze çarpan özellikleri şunlardır:
 
 <ol>
 <li>Gazlar, sürekli hareket halinde olan, düz çizgiler halinde hareket eden ve sadece diğer moleküllerle veya bir kabın duvarlarıyla çarpıştıklarında yön değiştiren parçacıklardan (atomlar veya moleküller) oluşur. 
 Standart sıcaklık ve basınçta bir argon gazı örneğini inceleyin. Hacmin sadece %0,01'inin, iki argon atomu arasında ortalama 3,3 nm'lik bir mesafeye (argonun atom yarıçapı 0,097 nm'dir) sahip atomlar tarafından kaplandığını göreceksiniz.Bu mesafe argonun kendi boyutundan çok daha büyüktür.</li>
 <li>Gazı oluşturan moleküller, aralarındaki mesafelere kıyasla ihmal edilebilir derecede küçüktür. Bu nedenle, tüm gaz parçacıklarının birleşik hacmi, kabın toplam hacmine göre önemsizdir. Parçacıklar, kütlesi olan fakat ihmal edilebilir hacme sahip "noktalar" olarak kabul edilirler. The particles are considered to be "points" that have mass but negligible volume.</li>
 <li>Bir gazın bir kaba uyguladığı basınç, gaz molekülleri ve kap duvarları arasındaki çarpışmalardan kaynaklanır.</li>
 <li>Gaz molekülleri birbirlerine veya konteyner duvarlarına çekici veya itici kuvvetler uygulamazlar; bu nedenle çarpışmaları elastiktir (enerji kaybını içermez). 
 Elastik çarpışmalar sırasında, çarpışan parçacıklar arasında enerji aktarılır. Bu nedenle parçacıkların ortalama kinetik enerjisi sabit kalır ve zamanla değişmez.</li>
 <li>Gaz moleküllerinin ortalama kinetik enerjisi, gazın kelvin sıcaklığı ile orantılıdır. 
 Tüm gazlar, moleküler kütlelerinden bağımsız olarak, aynı sıcaklıkta aynı ortalama kinetik enerjiye sahiptir.</li>
 </ol>
 
 Bu metin bu kaynaktan uyurlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/9-5-the-kinetic-molecular-theory"">Openstax, Chemistry 2e, Chapter 9.5 The Kinetic-Molecular Theory</a>.

Kinetik Moleküler Teori: Temel Varsayımlar

Ampirik olan ideal-gaz denklemi, gazların makroskopik özellikleri arasında ilişkiler kurarak davranışlarını tanımlar. İçin...

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JoVE Core

Kimya

Gases

Gazlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

kinetic molecular theory and gas behavior

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 is that gases are made of particles, either atoms or molecules, that move constantly. They travel in straight lines until they collide with other particles or with the walls of a container. A sample of argon gas at standard temperature and pressure shows that the particles take up only a tiny part of the total volume. The average distance between two argon atoms is much larger than the size of the atoms themselves. Because of this, gas particles are treated as points with mass but negligible volume.

Gas pressure comes from collisions between gas molecules and the walls of the container. The particles do not attract or repel each other, and they do not interact with the container walls through such forces. For that reason, their collisions are elastic, which means no energy is lost in the collision. Energy can still be transferred between colliding particles, but the average kinetic energy stays constant over time.

The average kinetic energy of gas particles depends on the kelvin temperature of the gas. It is proportional to temperature. At the same temperature, gases with different molecular masses have the same average kinetic energy.

Kinetic Molecular Theory and Gas Behavior

kinetic-molecular-theory-and-gas-behavior

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

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Pressure Units and Tools for Gas Measurement

Pressure is the force applied to a given area, and gas pressure comes from gas molecules colliding with surfaces. Each collision is tiny, but many collisions over a small area can create high pressure. Pressure increases when force increases or when the area gets smaller. It decreases when force drops or when the area gets larger. Pressure is measured in pascals, or Pa, in the SI system. One pascal equals 1 newton per square meter, and a newton is a unit of force equal to 1 kg·m/s2. A pascal...

gas laws: boyle's, gay-lussac, charles', avogadro's, and ideal gas law

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How Gas Pressure, Volume, and Temperature Change

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...

applications of the ideal gas law: molar mass, density, and volume

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Ideal Gas Law at STP and Gas Density

The ideal gas law links pressure, volume, number of moles, and temperature. It helps explain how gas volume changes when pressure or temperature changes. At standard temperature and pressure, or STP, the values are 273.15 K and 1 atm. At STP, one mole of an ideal gas occupies about 22.4 L. This is called the standard molar volume. The gas can be hydrogen, oxygen, argon, or carbon dioxide, and the volume is still about 22.4 liters. Half a mole occupies 11.2 L, and 2 moles occupy 44.8 L. The...

mixtures of gases: dalton's law of partial pressures and mole fractions

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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...

chemical stoichiometry and gases: using ideal gas law to determine moles

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Stoichiometry of Gases with the Ideal Gas Law

Chemical stoichiometry links the amounts of reactants and products in a chemical reaction. For gases, those amounts can also be measured by volume. If a gas’s volume, pressure, and temperature are known, the ideal gas equation can be used to find the number of moles present. The same idea works in reverse. If the moles of a gas are known, its volume can be found at any temperature and pressure. The transcript gives an example using 8.88 g of gallium reacting with excess hydrochloric acid.

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

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

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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...

kinetic molecular theory: molecular velocities, temperature, and kinetic energy

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Gas Particle Speed Distributions and Temperature

Gas particle speed distributions and temperature are key ideas in the kinetic molecular theory. This theory explains the gas laws by describing how gas molecules move, collide, and share energy. Gas molecules do not all move at the same speed. A gas sample has an average speed and an average kinetic energy, but individual molecules move at different speeds. Their collisions are elastic, which means momentum is conserved. Because so many molecules collide, the overall speed distribution stays...

behavior of gas molecules: molecular diffusion, mean free path, and effusion

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Gas Particle Motion, Diffusion, and Effusion

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real gases: effects of intermolecular forces and molecular volume deriving van der waals equation

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Real Gases: When the Ideal Gas Law Breaks Down

Real gases are gases that do not always follow the ideal gas law, PV = nRT, especially when pressure is high or temperature is low. The ideal gas model assumes gas particles have no attractive or repulsive forces and take up negligible space compared with the container. At room temperature and 1 atm or less, many gases behave close to ideally. When conditions change, the measured relationships between pressure, volume, and temperature can drift away from the ideal prediction. One way to see...

key terms and concepts

Explore how kinetic molecular theory explains gas pressure, particle motion, elastic collisions, and why average kinetic energy depends on kelvin temperature.

Kinetic Molecular Theory and Gas Behavior | JoVE K12

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Ohio’s Learning Standards and Model Curriculum

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CHEM1.PS1.5

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CH.6

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New York State Science Learning Standards

HS. Structure and Properties of Matter

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Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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Surface Tension, Capillary Action, and Viscosity

Surface Tension
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States of Matter and Phase Changes

The internal energy of a substance&#8212;the total kinetic energy of all its molecules and the potential energy of their associated forces&#8212;depends ...

Phase Transitions

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Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

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Heating and Cooling Curves

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Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

Use models to explain how changes in energy affect the arrangement and movement of the particles in solids, liquids, and gases, as well as the relative strengths of their intermolecular forces.

PS.Chm.7.1

Energy Basics

Chemical reactions, such as those that occur when you light a match, involve changes in energy as well as matter.

Chemical changes and their accompanying ...

First Law of Thermodynamics

Energy Conservation

Energy can be converted from one form into another, but all of the energy present before a change occurs always exists in some form ...

Internal Energy

The total of all possible kinds of energy present in a substance is called the internal energy (U), sometimes symbolized as E. Suppose a system with ...

Quantifying Heat

Thermal Energy&#160;

Microscopically, thermal energy is the kinetic energy associated with the random motion of atoms and molecules. Temperature is a ...

Quantifying Work

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Enthalpy

Chemists ordinarily use a property known as enthalpy (H) to describe the thermodynamics of chemical and physical processes. Enthalpy is defined as the sum ...

Thermochemical Equations

For a chemical reaction (the system) carried out at constant pressure &ndash; with the only work done caused by expansion or contraction &ndash; the ...

Constant Pressure Calorimetry

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Constant Volume Calorimetry

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Using Differential Scanning Calorimetry to Measure Changes in Enthalpy

Source: Laboratory of Dr. Terry Tritt &#8212; Clemson University
Differential Scanning Calorimetry (DSC) is a method of thermodynamic analysis based on ...

Hess's Law

There are two ways to determine the amount of heat involved in a chemical change: measure it experimentally, or calculate it from other experimentally ...

Standard Enthalpy of Formation

Enthalpy changes are typically tabulated for reactions in which both the reactants and products are at the same conditions. A standard state is a commonly ...

Enthalpies of Reaction

Hess&rsquo;s law can be used to determine the enthalpy change of any reaction if the corresponding enthalpies of formation of the reactants and products ...

Use mathematics and computational thinking to execute simple calorimetric calculations based on the Law of Conservation of Energy.

PS.Chm.7.2

Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

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Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

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Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

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Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

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Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

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Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

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Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

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Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many ...

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

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Ideal Gas Law

Source: Laboratory of Dr. Andreas Z&#252;ttel - Swiss Federal Laboratories for Materials Science and Technology
The ideal gas law describes the behavior ...

Derivation of the Ideal Gas Law
Gases are a fundamental state of matter. A gas is a collection of molecules that have a significant distance between their ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
	According to the ideal gas law for a given ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

Understand the relationship among pressure, temperature, volume, and phase.

Kinetic Molecular Theory and Gas Behavior

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