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

يحدد قانون معدل التفاعل العلاقة بين تركيز المادة المتفاعلة ومعدل التفاعل من حيث ثابت المعدل ، "k".
يصف ثابت المعدل العلاقة بين درجة الحرارة والمعلمات الحركية المتعلقة بالتصادم والاتجاه وطاقة التنشيط للجزيئات المتفاعلة عبر معادلة أرهينيوس. "A" هو ثابت يسمى عامل Arrhenius أو عامل التردد. "E" هو عامل أسي يدمج طاقة التنشيط المقاسة بالجول لكل مول ، وثابت الغاز ، ودرجة الحرارة بالكلفن.
يمكن تفسير اعتماد درجة حرارة المعلمات من خلال نموذج الاصطدام ، الذي ينص على أن الجزيئات المتفاعلة يجب أن تصطدم بطاقة كافية في الاتجاه الصحيح لبدء تفاعل كيميائي.
ويشكل عامل التردد مكونين هما تردد الاصطدام وعامل الاتجاه. تردد الاصطدام هو عدد الاصطدامات الجزيئية لكل وحدة زمنية ، بينما يصف عامل الاتجاه احتمال الاصطدامات ذات الاتجاه المناسب.
ومع ذلك ، فإن جزءا صغيرا فقط من الاصطدامات يؤدي إلى رد فعل. وذلك لأن الجزيئات المتفاعلة يجب أن تتغلب على حاجز الطاقة ، يسمى طاقة التنشيط ، لتتحول إلى منتجات.
فقط تلك الجزيئات التي تصطدم بطاقة حركية كافية سيكون لديها طاقة كامنة كافية لثني الروابط أو تمديدها أو كسرها لتتحول إلى وسيط عالي الطاقة يسمى الحالة الانتقالية ، أو المركب المنشط. يفقد المركب المنشط قصير العمر وغير المستقر الطاقة لتكوين منتجات مستقرة ، تكون طاقتها الإجمالية أقل من طاقة المواد المتفاعلة.
يمثل العامل الأسي في معادلة أرهينيوس جزء الاصطدامات الناجحة الناتجة عن المنتجات. تؤثر الزيادة في درجة الحرارة على كل من عامل التردد والعامل الأسي.
في درجات الحرارة المرتفعة ، تتحرك الجزيئات بشكل أسرع وأكثر قوة وطاقات حرارية أعلى ، مما يؤدي إلى تصادمات أكثر ملاءمة.
بالنسبة لمعظم التفاعلات ، تؤدي زيادة درجة الحرارة إلى ارتفاع التردد والعوامل الأسية ، مما يؤدي إلى ارتفاع ثابت المعدل ، وبالتالي يترجم إلى معدل تفاعل متسارع.

تأثير تغير درجة الحرارة على سرعة التفاعل

<div style="direction:rtl">

معادلة أرهينيوس,

<img alt="Figure1" src="/files/ftp_upload/11698/11698_Equation1.svg" style="text-align: center; height: 30px;">

يربط بين طاقة التنشيط وثابت السرعة k للعديد من التفاعلات الكيميائية.

في هذه المعادلة، R هو ثابت الغاز المثالي، الذي تبلغ قيمته 8.314 J/mol·K، T هي درجة الحرارة بالكلفن، Ea هي طاقة التنشيط بالجول لكل مول، e هو الثابت 2.7183، و A ثابت يسمى عامل التردد، ويرتبط بتكرار التصادمات واتجاه الجزيئات المتفاعلة.

يعكس عامل التردد، A، مدى تفضيل ظروف التفاعل للاصطدامات الموجهة بشكل صحيح بين الجزيئات المتفاعلة. تؤدي زيادة احتمال حدوث تصادمات موجهة بشكل فعال إلى قيم أكبر لـ A ومعدلات تفاعل أسرع.

يصف المصطلح الأسي، e−Eₐ/RT، تأثير طاقة التنشيط على سرعة التفاعل. وفقًا للنظرية الجزيئية الحركية، فإن درجة حرارة المادة هي مقياس لمتوسط الطاقة الحركية للذرات أو الجزيئات المكونة لها، فطاقة التنشيط المنخفضة تؤدي إلى جزء أكبر من الجزيئات النشطة بشكل كافٍ وتفاعل أسرع.

يصف المصطلح الأسي أيضًا تأثير درجة الحرارة على سرعة التفاعل. تمثل درجة الحرارة المرتفعة جزءًا أكبر من الجزيئات التي تمتلك طاقة كافية (RT) للتغلب على حاجز التنشيط (Ea). وهذا ينتج قيمة أعلى لثابت السرعة ومعدل تفاعل أسرع في المقابل.

الحد الأدنى من الطاقة اللازمة لتكوين منتج أثناء التصادم بين المواد المتفاعلة يسمى طاقة التنشيط (Ea). يعد الاختلاف في طاقة التنشيط المطلوبة والطاقة الحركية الناتجة عن تصادم الجزيئات المتفاعلة عاملاً أساسيًا يؤثر على سرعة التفاعل الكيميائي. إذا كانت طاقة التنشيط أكبر بكثير من متوسط الطاقة الحركية للجزيئات، فإن التفاعل سيحدث ببطء، حيث أن عددًا قليلاً فقط من الجزيئات سريعة الحركة سيكون لديها ما يكفي من الطاقة للتفاعل. إذا كانت طاقة التنشيط أصغر بكثير من متوسط الطاقة الحركية للجزيئات، فإن جزءًا كبيرًا من الجزيئات سيكون نشطًا بشكل كافٍ، وسيستمر التفاعل بسرعة.

تُستخدم مخططات التفاعل على نطاق واسع في الخواص الحركية الكيميائية لتوضيح الخصائص المختلفة لتفاعل معين. ويوضح كيف تتغير طاقة النظام الكيميائي أثناء خضوعه للتفاعل، وتحويل المواد المتفاعلة إلى منتجات.

هذا النص مقتبس من <a href="https://openstax.org/books/chemistry-2e/pages/12-5-collision-theory">Openstax, Chemistry 2e, Section 12.5: Collision Theory.</a>

</div>

معادلة أرهينيوس ،

يتعلق طاقة التنشيط وثابت المعدل ، k ، للعديد من التفاعلات الكيميائية.
في هذه المعادلة ، R هو الغاز المثالي ...

Education

JoVE Core

Organic Chemistry

الكيمياء العضوية

Unit 1

الوحدة الأولى

Thermodynamics and Chemical Kinetics

الديناميكا الحرارية والحركية الكيميائية

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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

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

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organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

Minnesota Academic Standards in Science

9-12

3.2.1 9C.3.1.1.2

Florida Department of Education

Physical Science

SC.912.P.12

SC.912.P.12.12

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relates the activation energy and the rate constant, k, for many chemical reactions.
In this equation, R is the ideal gas ...

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Arrhenius Equation in Reaction Speed

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