Name: heat changes in chemical equations
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 55 s
Channel: JoVE

K12 Standards

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

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.2

Thermochemical Equations

تحدث معظم التفاعلات الكيميائية عند الضغط الجوي. تحت ظروف الضغط المستمر،تغيير الحرارة المرتبط بالتفاعل دلتا Q،يساوي التغيير في المحتوى الحراري دلتا H،وتسمى أيضًا المحتوى الحراري أو حرارة التفاعل. المحتوى الحراري للتفاعل هو،الفرق بين المحتوى الحراري للنواتج والمواد المتفاعلة.عندما يكون المحتوى الحراري للنواتج أكبر من المحتوى الحراري للمواد المتفاعلة،تكون دلتا H موجبة. مثل هذه التفاعلات تمتص الحرارة وتكون ماصة للحرارة. على العكس من ذلك،إذا كان المحتوى الحراري للمواد المتفاعلة أكبر من المحتوى الحراري للنواتج،تكون دلتا H سالبة.مثل هذه التفاعلات تطلق الحرارة وتكون طاردة للحرارة. لأي تفاعل كيميائي،مقدار التغيير المصاحب في المحتوى الحراري،يعتمد على المقدار المكافئ من المواد المتفاعلة والنواتج،كما هو مبين بمعاملات المعادلة المتوازنة. المعادلة الكيميائية المتوازنة هي التي تشمل مراحل التسمية والمحتوى الحراري للتفاعل،دلتا H،و تسمى المعادلة الحرارية الكيميائية.لنضع في اعتبارنا،احتراق الميثان وهو مصدر أساسي للوقود. يطلق غاز الميثان المحترق الحرارة في المناطق المحيطة. الطبيعة الطاردة للحرارة للتفاعل يُشار إليها بالتغير السالب للمحتوى الحراري في المعادلة الحرارية الكيميائية.تظهر معادلة الاحتراق أنه،عندما يتفاعل مول واحد من غاز الميثان مع 2 مول من غاز الأكسجين،لإنتاج 1 مول من غاز ثاني أكسيد الكربون و 2 مول ماء سائل،فإنه يطلق حرارة 890.8 كيلو جول للمناطق المحيطة. النسبة المولية بين المواد المتفاعلة أو النواتج بالاضافة الي حرارة التفاعل،يمكن استخدامهما كعوامل تحويل لحساب الحرارة المتبادلة أثناء التفاعل. إذا كانت أسطوانة الغاز تحتوي على 25.5 كجم من الميثان،ويخضع كل غاز الميثان الموجود في الاسطوانة للاحتراق،ما هي كمية الحرارة التي سيتم إنتاجها؟بشكل عام،الخطة المفاهيمية هي تحويل الكتلة إلى مولات ثم المولات إلى حرارة التفاعل.للبدء،يتم ضرب 25.5 كجم في 1000 لإيجاد الكتلة بالجرام. ثم يتم قسمة كتلة الميثان على كتلتها المولية 16.0 جرام لكل مول للحصول على 1594 مول من الميثان. أخيرًا،باستخدام عامل التحويل بين مولات الميثان وحرارة التفاعل،1594 مول من الميثان يطلق 14.2 مرة و التي تمثل حرارة التفاعل.و تكون الاجابة بالسالب،لأن التفاعل طارد للحرارة،حيث تتدفق الحرارة في التفاعل.

<ol>
	<li>كاناجاراتنا ، سيباستيان ج. "مساعدة بصرية في حسابات المحتوى الحراري". مجلة التربية الكيميائية 77 ، العدد 9 (2000): 1178.</li>
	<li>كيفر ، ديفيد. "المحتوى الحراري والقانون الثاني للديناميكا الحرارية". مجلة التربية الكيميائية 96 ، العدد 7 (2019): 1407-1411.</li>
	<li>خليل ، معتصم I. "حساب المحتوى الحراري للتفاعل بطريقة المصفوفة". مجلة التربية الكيميائية 77 ، العدد 2 (2000): 185. 
	 </li>
</ol>

المعادلات الكيميائية الحرارية

بالنسبة إلى التفاعل الكيميائي (النظام) الذي يتم عند ضغط ثابت – مع العمل الوحيد الذي يتم نتيجة التوسع أو الانكماش – فإن المحتوى الحراري للتفاعل (الذي يسمى أيضاً حرارة التفاعل، ΔHrxn) يساوي الحرارة التي يتم تبادلها مع المحيط (qp).<img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-01.png" style="height: 40px;" />إن التغير في المحتوى الحراري هو خاصية شاملة، ويعتمد على كميات المواد المتفاعلة المشاركة في التفاعل (أو عدد المولات للمواد المتفاعلة). إن التغير في المحتوى الحراري خاص بالتفاعل، والحالات الفيزيائية لأنواع المادة المتفاعلة والمنتجات مهمة. يتميز التفاعل الطارد للحرارة بـ −ΔHrxn، بينما يكون للتفاعل الماص للحرارة +ΔHrxn value. نظراً لأن كمية الحرارة التي يتم إطلاقها أو امتصاصها بواسطة التفاعل تتطابق مع كمية كل مادة يتم استهلاكها أو إنتاجها بواسطة التفاعل، فمن الملائم استخدام معادلة كيميائية حرارية لتمثيل التغيرات في كل من المادة والطاقة. في المعادلة الكيميائية الحرارية، يظهر التغير في المحتوى الحراري للتفاعل على أنه ΔHrxn، ويتم تقديمه بشكل عام بعد معادلة التفاعل. يشير مقدار تكوّن ΔHrxn  إلى مقدار الحرارة المرتبطة بالتفاعل الموضح في المعادلة الكيميائية. تشير علامة ΔHrxn إلى ما إذا كان التفاعل طارد للحرارة أو ماص للحرارة، كما هو مكتوب. في المعادلة التالية، يتفاعل مول واحد من غاز الهيدروجين ونصف مول من غاز الأكسجين (عند درجة حرارة وضغط معينة) لتكوين مول واحد من الماء السائل (بنفس درجة الحرارة والضغط). <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-02.png" style="height: 40px;" />تشير هذه المعادلة إلى أن 286 كيلوجول من الحرارة قد تم  تحريرها في المحيط. بمعنى آخر، يتم  إطلاق 286 كيلوجول من الحرارة (التفاعل طارد للحرارة) لكل مول من الهيدروجين يتم استهلاكه أو لكل مول من الماء الذي يتم إنتاجه. وبالتالي، فإن المحتوى الحراري للتفاعل هو عامل تحويل يمكن استخدامه لحساب كمية الحرارة التي يتم إطلاقها أو امتصاصها أثناء التفاعلات التي تتضمن كميات محددة من المواد المتفاعلة والمنتجات. <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-03.png" style="height: 80px;" />إذا تم ضرب معاملات المعادلة الكيميائية في عامل ما (أي، إذا تم تغيير مقدار المادة)، فيجب ضرب التغير في المحتوى الحراري في هذا العامل نفسه. (زيادة بمقدار الضعف) <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-04.png" style="height: 40px;" />(انخفاض الكميات بمقدار الضعف) <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-05.png" style="height: 40px;" />لتوضيح أن التغير في المحتوى الحراري للتفاعل يعتمد على الحالات الفيزيائية للمواد المتفاعلة والنواتج، فكر في تكوّن الماء الغازي (أو بخار الماء). عندما يتفاعل مول واحد من غاز الهيدروجين و ½ مول من غاز الأكسجين لتكوين مول واحد من الماء الغازي، يتم إطلاق 242 كيلوجول فقط من الحرارة، مقابل 286 كيلوجول من الحرارة، التي يتم إطلاقها عندما يتكوّن الماء السائل. <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/799/799_Equations-06.png" style="height: 40px;" />

بالنسبة للتفاعل الكيميائي (النظام) الذي يتم إجراؤه عند ضغط ثابت - مع العمل الوحيد المنجز بسبب التمدد أو الانكماش - ...

Education

JoVE Core

الكيمياء

واحد

Thermochemistry

الكيمياء الحرارية

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

heat changes in chemical equations

Heat changes in chemical equations show how much energy a reaction releases or absorbs. At constant pressure, the enthalpy of reaction, or ΔHrxn, is equal to the heat exchanged with the surroundings, qp. Because this value depends on how much reactant takes part, it is an extensive property.

The size and sign of ΔHrxn also depend on the reaction itself and on the physical states of the substances involved. An exothermic reaction has a negative ΔHrxn value, while an endothermic reaction has a positive one. For that reason, a thermochemical equation is useful because it shows both the chemical change and the energy change together.

In a thermochemical equation, ΔHrxn is written after the chemical equation. Its magnitude tells how much heat is linked to the reaction as written. Its sign shows whether the reaction is exothermic or endothermic in that form.

For example, 1 mole of hydrogen gas and 1/2 mole of oxygen gas can react to form 1 mole of liquid water. This reaction releases 286 kJ of heat to the surroundings. That means 286 kJ is released for every mole of hydrogen used or every mole of water made, so ΔHrxn can act like a conversion factor.

If the coefficients in the chemical equation are multiplied, the enthalpy change must be multiplied by the same factor. A two-fold increase in the amounts gives a two-fold increase in ΔHrxn, and a two-fold decrease gives a two-fold decrease. The physical state matters too. When the same reaction makes gaseous water instead of liquid water, only 242 kJ of heat are released.

Heat Changes in Chemical Equations

energy basics

How Energy Changes in Chemical Reactions

Chemical reactions change matter and energy at the same time. A match lighting is a simple example. These energy changes are part of everyday life and appear in food, fuels, and industry. Food provides energy through metabolic reactions. The macronutrients in food break down and help keep the body functioning. Fuels such as gasoline, natural gas, and coal are burned to produce energy for transportation, heating, and electricity generation. Industrial chemical reactions also use large amounts...

first law of thermodynamics

Energy Conservation and Internal Energy

Energy conservation describes how energy changes form during chemical and physical changes. Energy can be converted from one form into another, but the energy present before a change still exists in some form after the change is complete. This is the law of conservation of energy. It says energy can neither be created nor destroyed. The law of conservation of matter also applies during chemical change. In most chemical reactions, the total amount of matter does not show a detectable change.

internal energy

Internal Energy, Heat, and Work

Internal energy is the total of all possible kinds of energy in a substance. It is often written as U, and sometimes as E. For a system that changes energy, the important value is the change in internal energy, or ΔU. ΔU is the difference between the final internal energy and the initial internal energy. The exact values of U final and U initial are usually not known, but the first law of thermodynamics only requires ΔU. A positive ΔU means the system gained energy from the surroundings. A...

quantifying heat

Heat Transfer and Specific Heat

Heat transfer and specific heat explain how thermal energy moves and how materials respond to it. Thermal energy is the kinetic energy linked to the random motion of atoms and molecules. Temperature is a measure of how hot or cold a substance is, and it depends on how much thermal energy those particles have. When atoms and molecules move or vibrate faster, their average kinetic energy is higher. That means the object has more thermal energy and a higher temperature. When they move more...

quantifying work

Pressure-Volume Work in Chemistry

Pressure-volume work shows how gas volume changes can transfer energy in chemistry. As a system changes, its internal energy may change too. Energy can move between the system and the surroundings through heat and work. Internal energy, heat, and work are related by an energy equation. Heat depends on a measured temperature change. Work depends on a measured change in volume called pressure-volume work. Work can be defined as a force acting through a distance. Pressure-volume work, also...

enthalpy

Enthalpy and Heat at Constant Pressure

Enthalpy describes heat changes in chemical and physical processes. Chemists use the symbol H for enthalpy. It is defined as a system’s internal energy, E, plus the product of pressure, P, and volume, V. Enthalpy is a state function, so only changes in enthalpy can be measured, not the enthalpy of a substance by itself. For many reactions, the pressure stays constant. Under those conditions, the enthalpy change, ΔH, can be written in a way that includes pressure-volume work. The term PΔV...

thermochemical equations

Heat changes in chemical equations show how much energy a reaction releases or absorbs. At constant pressure, the enthalpy of reaction, or ΔHrxn, is equal to the heat exchanged with the surroundings, qp. Because this value depends on how much reactant takes part, it is an extensive property. The size and sign of ΔHrxn also depend on the reaction itself and on the physical states of the substances involved. An exothermic reaction has a negative ΔHrxn value, while an endothermic reaction has a...

constant pressure calorimetry

Coffee Cup Calorimeter Heat Changes

Coffee cup calorimetry measures heat changes in reactions and physical changes using an insulated calorimeter. The calorimeter is calibrated and designed to limit heat exchange with the outside environment. That makes it possible to measure the heat taken in or released by a substance more accurately, including the energy content of foods. In calorimetry, the system is the substance or substances undergoing change. The surroundings are everything else inside the calorimeter, including the...

constant volume calorimetry

Bomb Calorimeter Heat Measurement

Bomb calorimetry measures the heat released by reactions that produce a lot of energy, especially combustion reactions. A coffee cup calorimeter works at constant pressure and is useful for reactions in solution. A bomb calorimeter works at constant volume and is used for reactions that make large amounts of heat and gaseous products. The word "bomb" refers to the strong, explosive force some reactions can have. In a bomb calorimeter, the volume does not change, so 94V = 0. That means the...

hess's law

Calculating Reaction Heat with Hess's Law

Calculating reaction heat with Hess's law lets chemists find enthalpy changes without measuring every reaction directly. Some reactions are hard or impossible to test in the lab. Even when a reaction can be measured, it is often easier to calculate the heat change from other known enthalpy values. Hess's law says that if a process can be written as the sum of several stepwise processes, the enthalpy change for the total process equals the sum of the enthalpy changes for the steps. This works...

standard enthalpy of formation

Using Standard Enthalpy Values in Chemistry

Enthalpy changes are often listed for reactions that start and end under the same conditions. Chemists use a standard state as a reference set of conditions for comparing properties. In IUPAC terms, the standard state means 1 bar of pressure and 1 M solutions, but it does not set a temperature. Many thermochemical tables still use 1 atm as the reference pressure. Because the difference between 1 bar and 1 atm is very small, enthalpy change usually stays almost the same. A superscripted o in...

enthalpies of reaction

Calculating reaction heat with Hess's law uses standard enthalpies of formation to find the enthalpy change of a reaction. When the formation values for the reactants and products are known, the overall reaction can be broken into simpler stepwise reactions. This approach helps show how the heat change for the full reaction is built from smaller parts. First, the reactants are thought of as being decomposed into their component elements. The enthalpy change for this step is proportional to the...

key terms and concepts

Learn how ΔHrxn shows heat released or absorbed in reactions, why equation coefficients matter, and how physical state changes the enthalpy value.

Heat Changes in Chemical Equations | JoVE K12

chemistry

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.

Matter and its Interactions

PS.Chm.4.1

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.8

IPC.8.B

Pennsylvania State Academic Standards

Physical Science

Chemical Reactions

3.2.9-12.D

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Tennessee Academic Standards

CHEM1.PS3.3

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CH.7

CH.7.a

CH.7.c

CHEM.13

CHEM.13.A

CHEM.13.C

Florida Department of Education

SC.912.P.10

SC.912.P.10.7

Georgia Standards of Excellence

SC3.

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PS.Chm.7.1

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Enthalpy

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Hess's Law

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Standard Enthalpy of Formation

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Understand the relationship among pressure, temperature, volume, and phase.

Heat Changes in Chemical Equations

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