Name: chemical equilibrium and kc rules
Uploaded: 2025-08-11T09:37:07.000Z
Duration: 3 min 10 s
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K12 Standards

north-carolina-k-12-science-standard-course-of-study

NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.5.2

The Equilibrium Constant

قانون فاعلية الكتلة يطرح ثابت التوازن للربط بين تركيزات التوازن للمواد المتفاعلة والنواتج. في معادلة كيميائية متزنة تكون فيها A وB مواد متفاعلة،وC وD نواتج،و بالأحرف الصغيرة a وb وc وd مُعاملات القياس المتكافئ للعناصر على التوالي،فإنّمعادلة ثابت التوازن تُعطى من خلال التركيزات المولية للنواتج،مقسومة على التركيزات المولية للمواد المتفاعلة،ويرفع الحاصل إلى قوة أسية تعادل معاملات القياس المتكافئ للمواد. غالبًا ما يُعبّر عن ثابت التوازن بالرمز K أو Kc،حيث الرمز السفلي c يدل على ثابت التوازن بالنسبة للتركيز المولي.لأنه يبين نسبة التركيزات المولية،فإن ثابت التوازن لا وحدة له. وجود ثابت توازن كبير يزيد على 1 يعني أن البسط،الذي هو تركيز النواتج،أكبر من المقام،الذي هو تركيز المواد المتفاعلة. يدل هذا على أن التوازن يميل نحو النواتج ويفضّل التفاعل الأمامي.وعلى العكس،وجود ثابت توازن صغير أقل بكثير من 1 يعني أن المقام أكبر من البسط. وهذا يدل على أن التوازن يميل نحو المواد المتفاعلة ويفضّل التفاعل العكسي. بالنسبة لثابت توازن يساوي 1 أو قريب منه تكون التركيزات النسبية للمواد المتفاعلة والنواتج متساوية تقريبًا.يدل هذا على أنه لا توجد بين التفاعل الأمامي أو العكسي،مفاضلة. إجراء تعديلات على المعادلة الكيميائية من شأنه أن يغير ثابت التوازن. إذا تم عكس تفاعل كيميائي ثابت توازنه يكون التعبير عن ثابت التوازن للتفاعل العكسي متبادل مع معادلة التفاعل الأمامي.وهكذا يكون ثابت التوازن الجديد يساوي 1 مقسومًا على إذا ضُربت المعامِلات في معامل آخر فإنّثابت التوازن يرفع لنفس المعامِل. و ثابت التوازن الجديد الآن سيكون مرفرع لأس(n)عند دمج تفاعلين منفصلين أو أكثر معاًيكون ثابت التوازن للتفاعل الإجمالي حاصل ضرب ثوابت التوازن المنفصلة. لذا يكون ثابت التوازن الجديد(y)مضروبة في في توازن غير متجانس،تُستثنى في معادلة ثابت التوازن المواد الصلبة والسوائل النقية.على سبيل المثال،في معادلة ثابت التوازن،الخاصة بتفكك نترات الأمونيوم الصلبة إلى غاز أكسيد النتروز وبخار الماء،تُستثنى نترات الأمونيوم-التي هي مادة صلبة نقية. يحدث هذا لأن التركيز المولي النسبي،لمادة صلبة أو سائلة نقية،يبقى ثابتًا أثناء التفاعل.

ثابت التوازن

ضع في اعتبارك أكسدة ثاني أكسيد الكبريت: <img alt="Eq1" src="/files/ftp_upload/11386/11386_Equation_1.png" style="text-align: center; height: 50px;" /> بالنسبة للتفاعل الذي يبدأ بخليط من المواد المتفاعلة فقط، يكون تركيز المنتج مبدئيًا مساويًا للصفر. مع تقدم التفاعل نحو التوازن في الاتجاه الأمامي، تنخفض تركيزات المادة المتفاعلة ويزداد تركيز المنتج. عند تحقيق التوازن ، تظل تركيزات المواد المتفاعلة والنواتج ثابتة. إذا بدأ التفاعل مع المنتجات الموجودة فقط ، يتقدم التفاعل نحو التوازن في الاتجاه العكسي. يتناقص تركيز المنتج بمرور الوقت وتزداد تركيزات المادة المتفاعلة حتى تصبح التركيزات ثابتة عند التوازن. ينص قانون تأثير الكتلة على أن نسبة تركيز المنتجات إلى تركيز المواد المتفاعلة عند التوازن ، والتي تم رفعها إلى معاملاتها المتكافئة ذات الصلة ، تساوي ثابتًا يسمى ثابت التوازن ،K أو Kc. وهكذا، فإن التعبير الثابت للتوازن للتفاعل أعلاه مكتوب على النحو التالي: <img alt="Eq2" src="/files/ftp_upload/11386/11386_Equation_2.png" style="text-align: center; height: 100px;" /> حيث أن، الرمز السفلي ‘c’ يشير إلى أن ثابت التوازن يأخذ في الاعتبار التركيز المولي للمواد المتفاعلة والمنتجات. يعكس مقدار ثابت التوازن بشكل صريح تكوين خليط التفاعل عند التوازن. سيصل التفاعل الذي يظهر K كبير إلى التوازن عندما يتم تحويل معظم المادة المتفاعلة إلى منتج ، بينما يشير K الصغير إلى أن التفاعل يحقق التوازن بعد تحويل القليل جدًا من المادة المتفاعلة . من’ المهم أن تضع في اعتبارك أن حجم Kلا يشير إلى مدى سرعة أو بطء الوصول إلى التوازن. يتم إنشاء بعض التوازنات بسرعة بحيث تكون فورية تقريبًا ، والبعض الآخر ببطء شديد بحيث لا يتم ملاحظة أي تغيير محسوس على مدار أيام أو سنوات أو أطول. يمكن استخدام ثابت التوازن للتفاعل للتنبؤ بسلوك المخاليط التي تحتوي على المواد المتفاعلة و / أو المنتجات. كما يتضح من عملية أكسدة ثاني أكسيد الكبريت الموصوفة أعلاه ، فإن التفاعل الكيميائي سيستمر في أي اتجاه ضروري لتحقيق التوازن. التوازن المزدوج تشتمل العديد من أنظمة التوازن على اثنين أو أكثر  من تفاعلات التوازن المقترنة  تلك التي تشترك في نوع واحد أو أكثر من أنواع المواد المتفاعلة أو المنتجات. يمكن أن ترتبط قيمة  K  لنظام يتضمن توازنات مقترنة بقيم  K  للتفاعلات الفردية. يتم تضمين ثلاث معالجات أساسية في هذا النهج، كما هو موضح أدناه: •يؤدي تغيير اتجاه المعادلة الكيميائية أساسًا إلى تبديل هويات “المتفاعلات” و “المنتجات,” وهكذا فإن ثابت التوازن للمعادلة المعكوسة هو ببساطة مقلوب للمعادلة الآجلة. • تغيير المعاملات المتكافئة في معادلة ببعض العوامل x ينتج عنه تغير أسي في ثابت التوازن بنفس العامل. • إضافة معادلتين أو أكثر من معادلات التوازن معًا ينتج عنها معادلة شاملة يكون ثابت التوازن هو الناتج الرياضي للتفاعل الفردي’s K قيم.تعبير ثابت للتوازن غير المتجانس بالنسبة إلى التوازن غير المتجانس ، الذي يتضمن المواد المتفاعلة والمنتجات في مرحلتين مختلفتين أو أكثر، لا يتم تضمين تركيزات المواد الصلبة النقية أو السوائل النقية في التعبير الثابت للتوازن ، كما هو موضح في المثال التالي: <img alt="Eq3" src="/files/ftp_upload/11386/11386_Equation_3.png" style="text-align: center; height: 150px;" /> وذلك لأن التركيزات النسبية للسوائل النقية والمواد الصلبة النقية تظل ثابتة أثناء التفاعل . تم اقتباس هذا النص من <a href="https://openstax.org/books/chemistry-2e/pages/13-2-equilibrium-constants">Openstax, Chemistry 2e, Section 13.2 Equilibrium Constants</a>.

ضع في اعتبارك أكسدة ثاني أكسيد الكبريت:

بالنسبة للتفاعل الذي يبدأ بمزيج من المواد المتفاعلة فقط ، يكون تركيز الناتج مساويا في البداية ل ...

Education

JoVE Core

الكيمياء

واحد

Chemical Equilibrium

الاتزان الكيميائي

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

chemical equilibrium and kc rules

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant.

A reaction can also begin with only products present. In that case, the reaction moves in reverse toward equilibrium. The product concentration falls with time, and the reactant concentrations rise until both become constant. This shows that a chemical reaction will move in whatever direction is needed to reach equilibrium.

The law of mass action links equilibrium to a constant value. It states that the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients, equals the equilibrium constant, K or Kc. The subscript c means the expression uses molar concentration. The size of K shows the mixture makeup at equilibrium. A large K means most reactant has changed to product before equilibrium is reached. A small K means only a little reactant changes to product. The value of K does not tell how fast equilibrium is reached.

Some equilibria form very quickly. Others take so long that no visible change may be seen for days, years, or longer. The equilibrium constant can still be used to predict how a mixture with reactants and/or products will behave. For coupled equilibria, two or more equilibrium reactions share one or more species. The K value for the overall system can be found from the K values of the separate reactions. Reversing a chemical equation changes K to its reciprocal. Multiplying the stoichiometric coefficients by a factor x changes K by that same factor as an exponent. Adding equilibrium equations gives an overall K equal to the product of the individual K values.

For heterogeneous equilibria, the reactants and products are in different phases. Pure solids and pure liquids are not included in the equilibrium constant expression. Their concentrations stay constant during the reaction, so they do not change the value of K. This rule is an important part of writing equilibrium expressions correctly.

Chemical Equilibrium and Kc Rules

the equilibrium constant

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant. A reaction can also begin with only products present. In that case, the reaction moves...

homogeneous equilibria for gaseous reactions

homogeneous-equilibria-for-gaseous-reactions

Relating Kc and Kp in Gas Equilibria

Gas-phase equilibrium can be written using either concentration or pressure. The equilibrium constant may be shown as Kc, which uses molar concentration, or as Kp, which uses partial pressure of the reactants and products. The link between Kc and Kp comes from the ideal gas equation and the definition of molarity. Molarity is the number of moles divided by volume. In the ideal gas equation, P stands for partial pressure, V for volume, n for number of moles, R for the gas constant, and T for...

le chatelier's principle: changing concentration

le-chatelier-s-principle-changing-concentration

Shifting Equilibrium by Changing Concentration

Chemical equilibrium is a dynamic balance. At equilibrium, the forward and reverse reactions happen at equal rates. If the system is stressed in a way that changes one rate more than the other, it is no longer at equilibrium and will shift until balance is restored. This behavior is described by Le Châtelier’s principle. Changes in concentration are a major stress on an equilibrium system. Reaction rates depend mainly on concentration and temperature. For that reason, changing the amount of a...

calculating the equilibrium constant

Finding Kc from Equilibrium Data

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction. One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to...

reaction quotient

Using Q to Track Equilibrium Changes

Reaction quotient Q helps track how far a reversible reaction has moved toward equilibrium. For a balanced reaction such as m A + n B ⇌ x C + y D, Q comes directly from the stoichiometric coefficients in the equation. When concentrations are used, the expression is written as Qc. For gases, a similar form uses partial pressures. These expressions use relative concentration and pressure values, not absolute values. That means reaction quotients are dimensionless and have no units. As a reaction...

dynamic equilibrium

Chemical Equilibrium in Reversible Reactions

Chemical equilibrium in reversible reactions happens when a reaction moves in both directions at the same time. A reversible reaction uses a double arrow to show that products can turn back into reactants. At equilibrium, the concentrations of reactants and products stay constant over time because the forward and reverse reaction rates are equal. The video uses the reversible decomposition of colorless dinitrogen tetroxide to brown nitrogen dioxide as an example. At time zero, there is finite...

calculating equilibrium concentrations

Equilibrium Concentrations from an ICE Table

Equilibrium concentrations can be found from initial concentrations and an equilibrium constant. This skill matters in many areas of science and technology, including pharmaceutical product formulation and dosing. After a drug is ingested or injected, it may take part in several chemical equilibria that change its final concentration in the body system of interest. Scientists use these quantitative equilibrium relationships to help calculate a dosage that will produce the desired therapeutic...

le chatelier's principle: changing volume (pressure)

le-chatelier-s-principle-changing-volume-pressure

Gas Equilibrium Under Volume Changes

Gas-phase equilibrium can shift when the volume of the system changes. In these reactions, a change in pressure changes concentration because the partial pressure of an ideal gas is proportional to its molar concentration. That means pressure changes affect equilibrium in the same way as concentration changes. When the volume of a gas mixture changes, the concentrations of reactants and products change together. Since every gas in the equilibrium occupies the same space, the same volume change...

le chatelier's principle: changing temperature

le-chatelier-s-principle-changing-temperature

Le Chatelier's Principle in Heating and Cooling

Le Chatelier's principle helps explain how chemical equilibrium responds to heating and cooling. A system at equilibrium will shift to restore balance after a temperature change, but the equilibrium constant, K, will not stay the same. Instead, the mixture reaches a new equilibrium with a different composition. This temperature effect is different from a concentration change, which shifts equilibrium without changing K. To understand why temperature matters, the reaction can be written with...

the small x assumption

Estimating Equilibrium with Small Changes

A small equilibrium constant can make equilibrium calculations easier. In these reactions, the equilibrium position favors the reactants. When the initial reactant concentration is high and the Kc value is small, the change in concentration may be negligible. In that case, the equilibrium concentration is close to the initial concentration. This idea helps simplify weak acid and weak base problems. Chemists can assume that some equilibrium concentrations are equal to the initial concentrations.

key terms and concepts

Explore chemical equilibrium, Kc, and the law of mass action. Learn how concentration changes, reaction direction, and mixed-phase equilibria shape equilibrium expressions.

Chemical Equilibrium and Kc Rules | JoVE K12

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JoVE Core Chemistry brings general chemistry concepts to life using concise and easy-to-understand animated video lessons. Plus, in the scientist-in-action videos, we demonstrate classical and original research experiments performed in today's laboratories worldwide.

Pennsylvania State Academic Standards

Physical Science

Chemical Reactions

3.2.9-12.F

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Arizona Science Standards

High School

HS+C.P1

HS+C.P1U1.6

Next Generation Science Standards

Matter and Its Interactions

HS-PS1-6

Florida Department of Education

SC.912.P.12

SC.912.P.12.13

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South Carolina College and Career Ready Science Standards

C-PS1-6

new-york-state-science-learning-standards

New York State Science Learning Standards

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PS.Chm.1.2

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The Energies of Atomic Orbitals

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PS.Chm.1.3

Periodic Classification of the Elements

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Molar Mass

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PS.Chm.2.1

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PS.Chm.2.2

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Chemical Equilibrium and Kc Rules

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