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

Boyle, Charles, Gay-Lussac ve Avogadro tarafından ortaya konan çeşitli gaz yasalarıyla ifade edilen farklı gaz özelliklerinin gözlemleri, kavramsal olarak kinetik moleküler teoriyi takip eder. Bir gazın uyguladığı basınç, sürekli hareket eden parçacıkların yer aldıkları kabın duvarları üzerindeki etkisinden kaynaklanır. Mol sayısı ve sıcaklığı sabit tutulurken, kabın hacminin küçültülmesi, gaz partiküllerini birbirine yaklaştırarak, partiküller arası boşluklarını azaltır.Bu daha küçük hacimde, gazın yoğunluğu ve çarpışma frekansı molekül-duvar çarpışmalarının sıklığı artar. Bu nedenle gazın uyguladığı basınç artar. Basınç ve hacim arasındaki ters ilişki Boyle yasasında verilmiştir.Sabit sıcaklıkta kaba daha fazla gaz molü eklemek, gaz yoğunluğunu ve dolayısıyla çarpışma sıklığını artırır. Başlangıç basıncını korumak için hacim genişlemelidir. Hacim ve moller arasındaki bu doğrudan ilişki Avogadro yasasında belirtilir.Şimdi, mol sayısının sabit tutulduğunu ve sıcaklığın yükseltildiğini düşünelim. Gaz parçacıklarının ortalama kinetik enerjisi sıcaklıkla orantılı olarak arttığı için parçacıklar daha sık ve kuvvetli bir şekilde çarpışır. Sıcaklık artarken hacim sabit tutulursa, gazın yoğunluğu ve çarpışma frekansı artar ve dolayısıyla basınç da artar.Basınç ve sıcaklık arasındaki doğrudan ilişki Gay-Lussac yasasında belirtilir. Öte yandan, basıncın sabit sayıda mol ile birlikte sabit kalması gerekiyorsa, çarpışmaları daha geniş bir yüzey alanına yaymak için sıcaklıktaki bir artışa hacimdeki artış eşlik etmelidir. Hacim ve sıcaklık arasındaki bu doğrudan ilişki Charles yasasında belirtilir.Son olarak, kinetik moleküler teoriye göre, gaz parçacıkları birbirlerini çekmez veya itmez. Farklı gazlardan oluşan bir karışımda, bileşenler bağımsız olarak hareket eder ve ayrı ayrı basınçları başka bir gazın varlığından etkilenmeden kalır. Karışımın toplam basıncı, bu nedenle, ayrı ayrı kısmi basınçların toplamıdır.Bu Dalton yasasıdır.

kinetik moleküler teori ve gaz yasaları

Kinetik moleküler teorinin (KMT) ve postülatlarının testi, bir gazın davranışını açıklama ve tanımlama yeteneğidir. Çeşitli gaz yasaları (Boyle, Charles, Gay-Lussac, Avogadro ve Dalton yasaları), kimyagerlerin teorinin varsayımlarının gaz moleküllerinin özelliklerini doğru bir şekilde temsil ettiğine inanmalarına neden olan KMT varsayımlarından türetilebilir.
 
 <h4>Kinetik Moleküler Teori Gazların Davranışını Açıklar</h4>
 
 Gaz basıncının hızla hareket eden gaz molekülleri tarafından uygulandığını ve doğrudan birim zaman başına duvarın birim alanına çarpan molekül sayısına bağlı olduğunu hatırlatan KMT, bir gazın davranışını kavramsal olarak şöyle açıklar:
 
 <ul>
 <li>Gay-Lussac yasası: Sıcaklık artarsa, gaz moleküllerinin ortalama hızı ve kinetik enerjisi artar. Hacim sabit tutulursa, gaz moleküllerinin artan hızı, kabın duvarları ile daha sık ve daha kuvvetli çarpışmalara neden olur, bu nedenle basıncı arttırır. Bu aynı zamanda Amontons Yasası olarak da bilinir.</li>
 <li>Bir gazın sıcaklığının artması durumunda, sabit basınç sadece gaz tarafından işgal edilen hacim artarsa korunabilir. Bu, moleküllerin konteyner duvarlarına ulaşmak için kat ettiği ortalama mesafelerin artmasına ve duvar yüzey alanının artmasına neden olacaktır. Bu koşullar, hem molekül-duvar çarpışmalarının sıklığını hem de birim alan başına çarpışma sayısını azaltacaktır, bunun birleşik etkileri, daha yüksek sıcaklıktaki daha büyük kinetik enerjiye bağlı olarak artan çarpışma kuvvetlerinin etkisini dengeleyecektir.</li>
 <li>Boyle yasası: Gaz hacmi azalırsa, konteyner duvar alanı azalır ve molekül-duvar çarpışma frekansı artar, her ikisi de gazın uyguladığı basıncı arttırır.</li>
 <li>Avogadro yasası: Sabit basınç ve sıcaklıkta, molekül-duvar çarpışmalarının sıklığı ve kuvveti sabittir. Bu koşullar altında, gaz halindeki moleküllerin sayısının arttırılması, artan çarpışma sıklığını telafi etmek için birim alan başına çarpışma sayısında bir azalma sağlamak için konteyner hacminde orantılı bir artış gerektirecektir.</li>
 <li>Dalton yasası: aralarındaki büyük mesafeler nedeniyle, karışımdaki bir gazın molekülleri, diğer gazların mevcut olup olmadığına bakılmaksızın, konteyner duvarlarına aynı frekansta çarpar ve bir gaz karışımının toplam basıncı, bireysel gazların (kısmi) basınçlarının toplamına eşittir.</li>
 </ul>
 
 Bu metin bu kaynaktan uyurlanmıştır: <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>

Kinetik Moleküler Teori ve Gaz Yasaları

Kinetik moleküler teorinin (KMT) ve varsayımlarının testi, bir gazın davranışını açıklama ve tanımlama yeteneğidir. Çeşitli gaz yasaları ...

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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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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...

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Ideal Gas Law at STP and Gas Density

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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

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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...

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

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Real Gases: When the Ideal Gas Law Breaks Down

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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.

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Gas Pressure Patterns in Kinetic Molecular Theory

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