Name: gas pressure patterns in kinetic molecular theory
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 34 s
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Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

De waarnemingen van verschillende gaseigenschappen, zoals uitgedrukt door de verschillende gaswetten afgeleid door Boyle, Charles, Gay-Lussac en Avogadro, volgen conceptueel uit de kinetische moleculaire theorie. De druk die door een gas wordt uitgeoefend, is het gevolg van de impact van constant bewegende deeltjes op de wanden van de container. Door het volume van de container te verkleinen, terwijl het aantal mol en de temperatuur constant blijft, worden de gasdeeltjes dichter bij elkaar gebracht, waardoor de onderlinge afstand tussen de deeltjes wordt verkleind.In dit kleinere volume neemt de dichtheid van het gas en de botsingsfrequentie de frequentie van botsingen tussen moleculen en wand toe. Daarom neemt de druk die door het gas wordt uitgeoefend toe. De omgekeerde relatie tussen druk en volume wordt gegeven door de wet van Boyle.Door bij constante temperatuur meer molen gas aan de container toe te voegen, neemt de gasdichtheid toe, en daarmee de botsingsfrequentie. Om de begindruk te behouden, moet het volume uitzetten. Deze directe relatie tussen volume en molen wordt gegeven door de wet van Avogadro.Bedenk nu dat het aantal mol constant wordt gehouden en de temperatuur wordt verhoogd. Omdat de gemiddelde kinetische energie van gasdeeltjes proportioneel toeneemt met de temperatuur, botsen de deeltjes vaker en krachtiger. Als het volume constant wordt gehouden terwijl de temperatuur wordt verhoogd, neemt de dichtheid van het gas en de botsingsfrequentie toe, en dus ook de druk.De directe relatie tussen druk en temperatuur wordt gegeven door de wet van Gay-Lussac. Als, aan de andere kant, de druk constant moet blijven samen met een constant aantal mol, dan moet een temperatuurstijging gepaard gaan door een toename van het volume om de botsingen over een groter oppervlak te spreiden. Deze directe relatie tussen volume en temperatuur wordt gegeven door de wet van Charles.Ten slotte, volgens de kinetische moleculaire theorie, trekken gasdeeltjes elkaar niet aan of stoten ze niet af. In een mengsel van verschillende gassen werken de componenten onafhankelijk en wordt hun individuele druk niet beïnvloed door de aanwezigheid van een ander gas. De totale druk van het mengsel is daarom de som van de individuele partiële drukken.Dit is de wet van Dalton.

kinetische molecuultheorie en gaswetten verklaren eigenschappen van gasmoleculen

De test van de kinetische moleculaire theorie (KMT) en haar postulaten is haar vermogen om het gedrag van een gas te verklaren en te beschrijven. De verschillende gaswetten (de wetten van Boyle, Charles, Gay-Lussac, Avogadro en Dalton) kunnen worden afgeleid uit de aannames van de KMT, die scheikundigen ertoe hebben gebracht te geloven dat de aannames van de theorie nauwkeurig de eigenschappen van gasmoleculen weergeven. <h4>De kinetische moleculaire theorie verklaart het gedrag van gassen</h4> Eraan herinnerend dat gasdruk wordt uitgeoefend door snel bewegende gasmoleculen en rechtstreeks afhangt van het aantal moleculen dat per tijdseenheid een oppervlakte-eenheid van de muur raakt, verklaart de KMT conceptueel het gedrag van een gas als volgt: <ul> <li>De wet van Gay-Lussac: Als de temperatuur stijgt, nemen de gemiddelde snelheid en kinetische energie van de gasmoleculen toe. Als het volume constant wordt gehouden, resulteert de verhoogde snelheid van de gasmoleculen in frequentere en krachtigere botsingen met de wanden van de container, waardoor de druk toeneemt. Dit wordt ook wel de wet van Amontons genoemd.</li> <li>Wet van Charles: Als de temperatuur van een gas toeneemt, kan een constante druk alleen worden gehandhaafd als het volume dat door het gas wordt ingenomen toeneemt. Dit zal resulteren in grotere gemiddelde afstanden die de moleculen afleggen om de containerwanden te bereiken, evenals in een groter wandoppervlak. Deze omstandigheden zullen zowel de frequentie van botsingen tussen moleculen als het aantal botsingen per oppervlakte-eenheid verminderen, waarvan de gecombineerde effecten het effect van verhoogde botsingskrachten als gevolg van de grotere kinetische energie bij de hogere temperatuur in evenwicht brengen.</li> <li>De wet van Boyle: Als het gasvolume afneemt, neemt het oppervlak van de containerwand af en neemt de botsingsfrequentie tussen molecuul en wand toe, waardoor de druk die door het gas wordt uitgeoefend toeneemt.</li> <li>De wet van Avogadro: Bij constante druk en temperatuur zijn de frequentie en kracht van botsingen tussen moleculen en muren constant. Onder dergelijke omstandigheden zal het vergroten van het aantal gasvormige moleculen een proportionele toename van het containervolume vereisen om een afname van het aantal botsingen per oppervlakte-eenheid te bewerkstelligen ter compensatie van de toegenomen frequentie van botsingen.</li> <li>Wet van Dalton: Vanwege de grote afstanden tussen hen bombarderen de moleculen van één gas in een mengsel de containerwanden met dezelfde frequentie, ongeacht of er andere gassen aanwezig zijn of niet, en de totale druk van een gasmengsel is gelijk aan de som van de ( partiële) druk van de afzonderlijke gassen.</li> </ul> Deze tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/9-5-the-kinetic-molecular-theory">Openstax, Chemistry 2e, Sectie 9.5: De kinetisch-moleculaire theorie.</a>

Kinetische molecuultheorie en gaswetten verklaren eigenschappen van gasmoleculen

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 ...

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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

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...

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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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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...

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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

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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...

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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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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Gas Pressure Patterns in Kinetic Molecular Theory

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