Name: arrhenius equation in reaction speed
Uploaded: 2023-04-30T18:28:32.000Z
Duration: 2 min 28 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-5

effect-of-temperature-change-on-reaction-rate

Effect of Temperature Change on Reaction Rate

Bir reaksiyonun hız yasası, bir reaktan konsantrasyonu ile reaksiyon hızı arasındaki ilişkiyi bir hız sabiti olan 'k' cinsinden tanımlar.
Hız sabiti, Arrhenius denklemi aracılığıyla reaksiyona giren moleküllerin çarpışması, yönelimi ve aktivasyon enerjisi ile ilgili sıcaklık ve kinetik parametreler arasındaki ilişkiyi tanımlar. 'A', Arrhenius faktörü veya frekans faktörü olarak adlandırılan bir sabittir. 'E', mol başına joule cinsinden ölçülen aktivasyon enerjisini, gaz sabitini ve Kelvin cinsinden sıcaklığı entegre eden üstel bir faktördür.
Parametrelerin sıcaklık bağımlılığı, reaksiyona giren moleküllerin kimyasal bir reaksiyonu başlatmak için doğru yönde yeterli enerji ile çarpışması gerektiğini belirten çarpışma modeli ile açıklanabilir.
Frekans faktörü iki bileşenden oluşur: çarpışma frekansı ve oryantasyon faktörü. Çarpışma frekansı, birim zamandaki moleküler çarpışma sayısıdır, oryantasyon faktörü ise olumlu bir oryantasyon ile çarpışma olasılığını tanımlar.
Yine de, çarpışmaların sadece küçük bir kısmı bir reaksiyona yol açar. Bunun nedeni, reaksiyona giren moleküllerin ürünlere dönüşmek için aktivasyon enerjisi adı verilen bir enerji bariyerini aşması gerektiğidir.
Yalnızca yeterli kinetik enerji ile çarpışan moleküller, geçiş durumu veya aktive edilmiş kompleks olarak adlandırılan yüksek enerjili bir ara ürüne dönüşmek için bağları bükmek, germek veya kırmak için yeterli potansiyel enerjiye sahip olacaktır. Kısa ömürlü, kararsız aktif kompleks, toplam enerjisi reaktanlarinkinden daha düşük olan kararlı ürünler oluşturmak için enerji kaybeder.
Arrhenius denklemindeki üstel faktör, ürünlerle sonuçlanan başarılı çarpışmaların oranını temsil eder. Sıcaklıktaki bir artış hem frekans faktörünü hem de üstel faktörü etkiler.
Yüksek sıcaklıklarda, moleküller daha hızlı, daha güçlü ve daha yüksek termal enerjilerle hareket eder ve bu da daha uygun çarpışmalara yol açar.
Çoğu reaksiyon için, bir sıcaklık artışı daha yüksek frekans ve üstel faktörlerle sonuçlanır, bu da hız sabitinde bir artışa yol açar ve sonuç olarak hızlandırılmış bir reaksiyon hızına dönüşür.

sıcaklık değişiminin reaksiyon hızına etkisi

Arrhenius denklemi,

<img alt="Figure1" src="/files/ftp_upload/11698/11698_Equation1.svg" style="text-align: center; height: 30px;">

Birçok kimyasal reaksiyon için aktivasyon enerjisi ile hız sabiti k arasında ilişki kurar.

 Bu denklemde R, 8,314 J/mol·K değerine sahip ideal gaz sabitidir, T kelvin cinsinden sıcaklıktır, E_a mol başına joule cinsinden aktivasyon enerjisidir, e 2,7183 sabitidir ve A bir sabittir çarpışmaların sıklığı ve reaksiyona giren moleküllerin yönelimi ile ilgili olan frekans faktörü olarak adlandırılır.

Frekans faktörü A, reaksiyon koşullarının reaktant molekülleri arasındaki doğru yönlendirilmiş çarpışmaları ne kadar iyi desteklediğini yansıtır. Etkili yönlendirilmiş çarpışma olasılığının artması, A için daha büyük değerlere ve daha hızlı reaksiyon hızlarına neden olur.

Üstel terim, e−Eₐ/RT, aktivasyon enerjisinin reaksiyon hızı üzerindeki etkisini açıklar. Kinetik moleküler teoriye göre, maddenin sıcaklığı, onu oluşturan atomların veya moleküllerin ortalama kinetik enerjisinin bir ölçüsüdür; daha düşük bir aktivasyon enerjisi, yeterince enerjilendirilmiş moleküllerin daha önemli bir fraksiyonuna ve daha hızlı bir reaksiyona neden olur.

Üstel terim ayrıca sıcaklığın reaksiyon hızı üzerindeki etkisini de açıklar. Daha yüksek bir sıcaklık, aktivasyon bariyerini (E_a) aşmak için yeterli enerjiye (RT) sahip olan moleküllerin buna karşılık daha büyük bir kısmını temsil eder. Bu, hız sabiti için daha yüksek bir değer ve buna bağlı olarak daha hızlı bir reaksiyon hızı sağlar.

Reaksiyona giren maddeler arasındaki çarpışma sırasında bir ürün oluşturmak için gereken minimum enerjiye aktivasyon enerjisi (E_a) denir. Gerekli aktivasyon enerjisi ile reaksiyona giren moleküllerin çarpışmasıyla sağlanan kinetik enerji arasındaki fark, kimyasal reaksiyonun hızını etkileyen birincil faktördür. Aktivasyon enerjisi moleküllerin ortalama kinetik enerjisinden çok daha büyükse, yalnızca hızlı hareket eden birkaç molekül reaksiyona girmeye yetecek enerjiye sahip olacağından reaksiyon yavaş gerçekleşecektir. Aktivasyon enerjisi moleküllerin ortalama kinetik enerjisinden çok daha küçükse, moleküllerin büyük bir kısmı yeterince enerjik olacak ve reaksiyon hızla ilerleyecektir.

Reaksiyon diyagramları, ilgilenilen bir reaksiyonun çeşitli özelliklerini göstermek için kimyasal kinetikte yaygın olarak kullanılmaktadır. Bir kimyasal sistemin enerjisinin, reaksiyona girerken nasıl değiştiğini, reaktantları ürünlere dönüştürdüğünü gösterir.

Bu metin ABC’den uyarlanmıştır<a href="https://openstax.org/books/chemistry-2e/pages/12-5-collision-theory">Openstax, Chemistry 2e, Section 12.5: Collision Theory.</a>

Sıcaklık Değişiminin Reaksiyon Hızına Etkisi

Arrhenius denklemi,

Birçok kimyasal reaksiyon için aktivasyon enerjisini ve hız sabitini (k) ilişkilendirir.
Bu denklemde, R ideal gazdır ...

Education

JoVE Core

Organic Chemistry

Organik Kimya

Unit 1

Ünite 1

Thermodynamics and Chemical Kinetics

Termodinamik ve Kimyasal Kinetik

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

arrhenius equation in reaction speed

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster.

In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor.

The frequency factor, A, describes how often reacting molecules collide and how well they are oriented during those collisions. Better orientation increases the chance of effective collisions. That leads to larger A values and faster reaction rates.

The exponential term, e−Ea/RT, shows how activation energy affects the reaction rate. Kinetic molecular theory says that temperature measures the average kinetic energy of atoms or molecules. When activation energy is lower, more molecules have enough energy to react, and the reaction is faster.

The same exponential term also shows the effect of temperature. At higher temperature, a larger fraction of molecules has enough energy, RT, to get over the activation barrier, Ea. This increases the rate constant and speeds up the reaction.

Activation energy is the minimum energy needed to form products during a collision between reactants. If Ea is much larger than the average kinetic energy of the molecules, only a few fast-moving molecules can react, so the reaction is slow. If Ea is much smaller than the average kinetic energy, many molecules can react, so the reaction proceeds quickly.

Reaction diagrams are often used in chemical kinetics to show how a system’s energy changes as reactants turn into products. They help visualize the energy barrier and the path from reactants to products. This text is adapted from Openstax, Chemistry 2e, Section 12.5: Collision Theory.

Arrhenius Equation in Reaction Speed

chemical reactions

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effect of temperature change on reaction rate

The Arrhenius equation connects activation energy, temperature, and the rate constant, k, for many chemical reactions. It helps explain why some reactions move slowly while others happen faster. In this equation, R is the ideal gas constant, with a value of 8.314 J/mol·K. T is the temperature in kelvin, Ea is the activation energy in joules per mole, e is the constant 2.7183, and A is the frequency factor. The frequency factor, A, describes how often reacting molecules collide and how well...

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key terms and concepts

Explore how the Arrhenius equation links temperature, activation energy, and collision orientation to reaction speed in high school chemistry.

Arrhenius Equation in Reaction Speed | JoVE K12

organic chemistry

JoVE Core Organik Kimya, kısa ve anlaşılması kolay animasyonlu video dersleri kullanarak stereokimya, reaksiyonlar ve mekanizmaların temel kavramlarını açıklar. Buna ek olarak, bilim insanlarının yer aldığı videolar, ilgili kavramların günümüz laboratuvarlarında gerçekleştirilen klasik ve orijinal araştırma deneylerinde nasıl uygulandığını göstermektedir.

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9-12

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Florida Department of Education

Physical Science

SC.912.P.12

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Arrhenius Equation in Reaction Speed

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