Name: how reactant concentration sets reaction rate
Uploaded: 2025-05-22T09:05:33.000Z
Duration: 2 min 33 s
Channel: JoVE

K12 Standards

Florida Department of Education

High School

Physical Science

SC.912.P.12

SC.912.P.12.12

Rate Law and Reaction Order

بالنسبة لأي تفاعل ، يمكن التعبير عن العلاقة بين معدل التفاعل وتركيزات المادة المتفاعلة رياضيا باستخدام قانون المعدل أو معادلة المعدل. 
في قانون المعدل ، "k" هو ثابت التناسب ، أو ثابت المعدل ، و "n" هو ترتيب التفاعل بالنسبة إلى متفاعل واحد ، غالبا ما تكون قيمته عددا صحيحا. في قوانين المعدل للتفاعلات متعددة المواد المتفاعلة ، فإن ترتيب التفاعل الكلي هو مجموع جميع أوامر المتفاعلات.
لكل مادة متفاعلة ، يتم تحديد معدل التفاعل وثابت المعدل والتركيز وترتيب التفاعل تجريبيا.
عادة ما تأخذ الأوامر المتفاعلة الفردية القيم 0 أو 1 أو 2 ، وبناء على ترتيب التفاعل الكلي ، يمكن تصنيف التفاعلات الكيميائية على أنها تفاعلات من الدرجة الصفرية أو الأولى أو من الدرجة الثانية.
التفاعل الكيميائي أحادي المتفاعل أو غير الجيلي الذي يظل معدل التفاعل ثابتا طوال مدته هو تفاعل من الرتبة الصفرية. ترتيب المادة المتفاعلة في تفاعل الرتبة الصفرية يساوي صفرا، ويرتفع تركيز المادة المتفاعلة إلى قوة الصفر.
نظرا لأن قيمة أي عدد مرفوعة إلى قوة الصفر تساوي واحدا، فإن معدل تفاعل الرتبة الصفرية يساوي ثابت المعدل، وبالتالي فهو مستقل عن تركيز المادة المتفاعلة.
التفاعل الكيميائي أحادي الجزيء حيث يتناسب معدل التفاعل طرديا مع تركيز المادة المتفاعلة هو تفاعل من الدرجة الأولى. ترتيب المتفاعل لتفاعل الدرجة الأولى هو واحد ، ووفقا لقانون المعدل ، يتم رفع تركيز المادة المتفاعلة إلى القوة الأولى.
نظرا لأن قيمة أي رقم مرفوع إلى قوة واحد تظل كما هي ، فإن معدل تفاعل تفاعل الدرجة الأولى يعتمد بشكل مباشر على تركيز المادة المتفاعلة. مع انخفاض تركيز المادة المتفاعلة ، ينخفض معدل التفاعل بشكل متناسب بطريقة خطية.
التفاعل الكيميائي أحادي الجزيء حيث يعتمد معدل التفاعل على مربع تركيز المادة المتفاعلة هو تفاعل من الدرجة الثانية. مع انخفاض تركيز المادة المتفاعلة ، ينخفض معدل التفاعل بشكل كبير بطريقة تربيعية.

قانون معدل التفاعل ورتبة التفاعل

<div style="direction:rtl">

تتأثر سرعة التفاعل بتركيزات المواد المتفاعلة. قوانين المعدلات (قوانين المعدلات التفاضلية) أو معادلات معدل التفاعل هي تعبيرات رياضية تصف العلاقة بين سرعة التفاعل الكيميائي وتركيز المواد المتفاعلة.
على سبيل المثال، في تفاعل عام aA + bB ⟶ المنتجات، حيث a و b عبارة عن معاملات تكافؤية، يمكن كتابة قانون السرعة على النحو التالي:

معدل التفاعل = k[A]m[B]n

يمثل [A] و[B] التركيزات المولية للمواد المتفاعلة، وk هو ثابت السرعة، وهو خاص بتفاعل معين عند درجة حرارة معينة.

الأسس m و n هما رتبة التفاعل وعادةً ما يكونان أعدادًا صحيحة موجبة، على الرغم من أنها يمكن أن تكون كسورًا أو قيمًا سالبة أو صفرًا.

يتم تحديد ثابت السرعة k ورتب التفاعل m وn تجريبيًا من خلال ملاحظة كيفية تغير سرعة التفاعل مع تغير تركيزات المواد المتفاعلة. ثابت السرعة k لا يعتمد على تركيزات المواد المتفاعلة ولكنه يختلف باختلاف درجة الحرارة.

تصف رتب التفاعل في قانون السرعة الاعتماد الرياضي للسرعة على تركيزات المواد المتفاعلة. بالرجوع إلى قانون السرعة العام (المعدل = k[A]m[B]n)، يكون التفاعل من الرتبة m بالنسبة إلى A والرتبة n بالنسبة إلى B. على سبيل المثال، إذا كانت m = 1 وn = 2، فإن التفاعل يكون من الرتبة الأولى بالنسبة إلى A ومن الرتبة الثانية بالنسبة إلى B. إجمالي رتبة التفاعل هو ببساطة مجموع الرتب لكل مادة متفاعلة. بالنسبة لمثال قانون المعدل هنا، يكون التفاعل كليًا من الدرجة الثالثة (1 + 2 = 3).

النهج التجريبي الشائع لتحديد قوانين المعدلات هو طريقة المعدلات الأولية. تتضمن هذه الطريقة قياس معدلات التفاعل لتجارب تجريبية متعددة يتم إجراؤها باستخدام تركيزات متفاعلة أولية مختلفة. تسمح مقارنة المعدلات المقاسة لهذه التجارب بتحديد رتب التفاعل، وبالتالي ثابت السرعة، والتي تستخدم معًا لصياغة قانون السرعة.

قد تظهر قوانين السرعة رتبًا جزئية لبعض المواد المتفاعلة، ويتم ملاحظة رتب التفاعل السلبية في بعض الأحيان عندما تؤدي الزيادة في تركيز أحد المواد المتفاعلة إلى انخفاض في سرعة التفاعل. من المهم أن نلاحظ أن قوانين السرعة يتم تحديدها عن طريق التجربة فقط ولا يمكن التنبؤ بها بشكل موثوق من خلال تكافؤ التفاعل.
تحدد رتبة التفاعل العلاقة بين سرعة التفاعل وتركيز المواد المتفاعلة أو المنتجات.

<ul style="padding-right: 35px; list-style-type: disc;">
	<li style="text-align: right;">في التفاعل من الرتبة الصفرية، ليس لتركيز المواد المتفاعلة أي تأثير على سرعة التفاعل، الذي يظل ثابتًا طوال الوقت.</li>
	<li style="text-align: right;">في التفاعل من الرتبة الأولى، تتناسب سرعة التفاعل بشكل مباشر وطرديًا مع التغير في تركيز المادة المتفاعلة. كلما انخفض تركيز المادة المتفاعلة، انخفض معدل التفاعل أيضًا بشكل تناسبي.</li>
	<li style="text-align: right;">في التفاعلات من الرتبة الثانية أو التفاعلات ذات الرتب الأعلى، تتناسب سرعة التفاعل مع القيمة الأسية للمواد المتفاعلة. لذلك، مع تقدم التفاعل وانخفاض تركيز المواد المتفاعلة، تنخفض سرعة التفاعل بشكل كبير.</li>
</ul>

هذا النص مقتبس من <a href="https://openstax.org/books/chemistry-2e/pages/12-3-rate-laws#57033">Openstax, Chemistry 2e, Section 12.3: Rate Laws</a>.

</div>

يتأثر معدل التفاعل بتركيزات المواد المتفاعلة. قوانين المعدل (قوانين المعدل التفاضلي) أو معادلات المعدل هي تعبيرات رياضية ...

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

how reactant concentration sets reaction rate

Reaction rate depends on reactant concentration, and rate laws show that relationship with a mathematical equation. A rate law, also called a differential rate law or rate equation, links the rate of a chemical reaction to the concentrations of its reactants.

For a generic reaction, a A + b B  products, the rate law can be written as rate = k [A]^m [B]^n. Here, [A] and [B] are the molar concentrations of the reactants. The constant k is the rate constant, and it is specific to one reaction at a specific temperature.

The exponents m and n are the reaction orders. They are usually positive integers, but they can also be fractions, negative values, or zero. If m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is the sum of the separate orders, so this example is third order overall.

Rate law values are found by experiment, not by stoichiometry. Scientists change the initial reactant concentrations in several trials and measure the reaction rate. This method, called the method of initial rates, helps determine the reaction orders and then the rate constant.

Some reactions show zero-order behavior. In a zero-order reaction, changes in reactant concentration do not change the rate, so the rate stays constant. In a first-order reaction, the rate changes in direct proportion to the reactant concentration. In second-order and higher-order reactions, the rate depends on the concentration raised to an exponent, so the rate drops more sharply as reactants are used up.

Rate laws can also show fractional orders, and some can even show negative orders. A negative order means that increasing one reactant can decrease the reaction rate. These patterns are useful for describing how reaction rate changes in real experiments. They are not reliably predicted from the reaction equation alone, so the rate law must be determined experimentally.

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C. The Law of Universal Gravitation states that gravitational forces act on all objects irrespective of their size and position.

D. Gases consist of great numbers of molecules moving in all directions. The behavior of gases can be modeled by the kinetic molecular theory.

E. Chemical reaction rates change with conditions under which they occur. Chemical equilibrium is a dynamic state in which forward and reverse processes occur at the same rates.

How Reactant Concentration Sets Reaction Rate

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