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

Während die Gasgesetze die Beziehungen zwischen verschiedenen Eigenschaften idealer Gase zusammenfassen, erklärt die kinetische Gastheorie warum Gase bestimmten Gesetzen folgen. Die Theorie basiert auf einigen wenigen Annahmen oder Postulaten. Die erste Annahme ist, dass Gasteilchen von vernachlässigbarer Größe sind.Ein Gas ist meist ein leerer Raum, der aus kleinen Teilchen besteht, die in weit größeren Abständen als ihre eigenen Dimensionen voneinander getrennt sind. Ihr gemeinsames Volumen ist vernachlässigbar im Verhältnis zum Gesamtvolumen, in dem das Gas enthalten ist. Im Gegensatz zu Feststoffen und Flüssigkeiten, die aufgrund ihrer kleinen Teilchenabstände nicht verdichtbar sind, sind Gase hoch verdichtbar.Gasteilchen befinden sich in einem konstantem Zustand der Bewegung entlang gerader Linien in zufälligen Richtungen. Ihre Wege ändern sich nur, wenn sie mit anderen Teilchen oder mit den Wänden ihres Behälters kollidieren. Die zweite Annahme ist, dass die Gasteilchen perfekt elastische Kollisionen haben.Sie kollidieren und prallen voneinander ab ohne zusammenzukleben. Dies kann man mit den Kollisionen zwischen Billardkugeln während eines Billardspiels vergleichen. Wenn Gasteilchen kollidieren, tauschen sie Energie miteinander aus, aber es gibt keinen Nettoverlust an Energie.Mit anderen Worten, die Gesamtenergie des Systems bleibt konstant. Gasteilchen sind ständig in Bewegung;daher besitzen sie kinetische Energie. So besagt die dritte Annahme, dass die durchschnittliche kinetische Energie eines Gases zu seiner absoluten Temperatur in Kelvin proportional ist.Das bedeutet, dass die kinetische Energie mit der Temperatur zunimmt, und folglich bewegen sich die Teilchen schneller. Bei höheren Temperaturen nimmt ihre Geschwindigkeit zu. Umgekehrt, wenn die Temperatur fällt, nimmt auch die kinetische Energie der Partikel ab und sie bewegen sich langsamer.Bei einer gegebenen Temperatur, alle Gase, unabhängig von ihrer molekularen Masse, haben die gleiche durchschnittliche kinetische Energie. Die kinetische Energie ist gleich der Masse mal Geschwindigkeit zum Quadrat. Damit die verschiedenen Gase die gleiche durchschnittliche kinetische Energie haben, müssen ihre Gasteilchen sich mit unterschiedlichen Durchschnittsgeschwindigkeiten bewegen.Schwerere Gase haben daher geringere Durchschnittsgeschwindigkeiten, während leichtere Gase höhere Durchschnittsgeschwindigkeiten haben. Zum Beispiel, haben Helium und Neon, bei der gleichen Temperatur die gleiche durchschnittliche kinetische Energie. Aufgrund des Unterschiedes in ihren Massen bewegen sich die Neonatome viel langsamer als die Heliumatome.

grundpostulate der kinetischen molekültheorie: teilchengröße, energie und kollision

Die empirische Idealgasgleichung beschreibt das Verhalten von Gasen, indem sie Beziehungen zwischen ihren makroskopischen Eigenschaften herstellt. Das Gesetz von Charles besagt beispielsweise, dass Volumen und Temperatur in direktem Zusammenhang stehen. Gase dehnen sich daher aus, wenn sie bei konstantem Druck erhitzt werden. Obwohl die Gasgesetze erklären, wie sich die makroskopischen Eigenschaften relativ zueinander ändern, erklären sie nicht den Grund dafür. Die kinetische Molekulartheorie ist ein mikroskopisches Modell, das hilft zu verstehen, was mit Gaspartikeln auf molekularer oder atomarer Ebene passiert, wenn sich Bedingungen wie Druck oder Temperatur ändern. Im Jahr 1857 veröffentlichte Rudolf Clausius eine vollständige und zufriedenstellende Form der Theorie, die die verschiedenen Gasgesetze durch die Postulate, die auf der Grundlage Hunderter experimenteller Beobachtungen des Verhaltens von Gasen entwickelt wurden, effektiv erklärt. Die hervorstechenden Merkmale dieser Theorie sind: <ol> <li>Gase bestehen aus Teilchen (Atomen oder Molekülen), die sich in ständiger Bewegung befinden, sich in geraden Linien fortbewegen und ihre Richtung nur ändern, wenn sie mit anderen Molekülen oder mit den Wänden eines Behälters kollidieren. Untersuchen Sie eine Argongasprobe bei Standardtemperatur und -druck. Es zeigt, dass nur 0,01 % des Volumens von Atomen mit einem durchschnittlichen Abstand von 3,3 nm (Atomradius von Argon beträgt 0,097 nm) zwischen zwei Argonatomen eingenommen werden. Der Abstand ist weitaus größer als seine eigene Dimension.</li> <li>Die Moleküle, aus denen das Gas besteht, sind im Vergleich zu den Abständen zwischen ihnen vernachlässigbar klein. Daher ist das Gesamtvolumen aller Gaspartikel im Verhältnis zum Gesamtvolumen des Behälters vernachlässigbar. Die Teilchen werden als „Punkte“ betrachtet, die eine Masse, aber ein vernachlässigbares Volumen haben.</li> <li>Der Druck, den ein Gas in einem Behälter ausübt, entsteht durch Kollisionen zwischen den Gasmolekülen und den Behälterwänden.</li> <li>Gasmoleküle üben keine anziehenden oder abstoßenden Kräfte aufeinander oder auf die Behälterwände aus; daher sind ihre Kollisionen elastisch (sie gehen nicht mit einem Energieverlust einher). Bei elastischen Stößen wird Energie zwischen den kollidierenden Teilchen übertragen. Die durchschnittliche kinetische Energie der Teilchen bleibt daher konstant und ändert sich nicht mit der Zeit.</li> <li>Die durchschnittliche kinetische Energie der Gasmoleküle ist proportional zur Kelvin-Temperatur des Gases. Alle Gase haben unabhängig von ihrer Molekülmasse bei gleicher Temperatur die gleiche durchschnittliche kinetische Energie.</li> </ol> Dieser Text wurde angepasst von <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>.

Grundpostulate der kinetischen Molekültheorie: Teilchengröße, Energie und Kollision

Die empirische Ideal-Gas-Gleichung beschreibt das Verhalten von Gasen, indem sie Beziehungen zwischen ihren makroskopischen Eigenschaften herstellt. Für...

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KEY TERMS AND CONCEPTS

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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

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

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

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

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

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

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

kinetic-molecular-theory-gas-laws-explain-properties-gas

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

Gas particle motion, diffusion, and effusion explain how gases spread and escape in everyday settings. Gas molecules move at very high speeds, but they collide with other gas molecules and change direction many times before reaching a target. At room temperature, a gas molecule can experience billions of collisions each second. The mean free path is the average distance a molecule travels between collisions. This distance becomes larger when pressure decreases. In general, the mean free path...

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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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
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

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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

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

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

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

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Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

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

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

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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

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

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Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

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

As a system undergoes a change, its internal energy can change, and energy can be transferred from the system to the surroundings, or from the ...

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

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a ...

Constant Volume Calorimetry

Calorimeters are useful to determine the heat released or absorbed by a chemical reaction. Coffee cup calorimeters are designed to operate at constant ...

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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

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

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

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

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

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

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

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

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

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

In addition to measuring quantities ...

The ideal-gas equation, which is empirical, describes the behavior of gases by establishing relationships between their macroscopic properties. For ...

Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws ...

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

The kinetic molecular theory qualitatively explains the behaviors described by the various gas laws. The postulates of this theory may be applied in a ...

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

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and ...

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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