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

Die meisten chemischen Reaktionen finden bei atmosphärischem Druck statt. Unter Bedingungen konstanten Drucks, die mit der Reaktion verbundene Wärmeänderung delta Q, ist gleich der Änderung der Enthalpie Delta H, auch die Enthalpie oder Reaktionswärme genannt. Die Enthalpie der Reaktion ist der Unterschied zwischen den Enthalpien der Produkte und den Reaktanten.Wenn die Enthalpie der Produkte größer als die Enthalpie der Reaktanten ist, ist delta H positiv. Solche Reaktionen absorbieren Wärme und sind endotherm. Im Gegenteil, wenn die Enthalpie der Reaktanten größer als die Enthalpie der Produkte ist, ist delta H negativ.Solche Reaktionen setzen Wärme frei und sind exotherm. Für jede chemische Reaktion, die Größenordnung der begleitenden Enthalpieänderung hängt von den stöchiometrischen Mengen der Reaktanten und Produkte ab, angegeben durch die Koeffizienten der ausgeglichenen Gleichung. Eine ausgeglichene chemische Gleichung, die Phasenübergänge und Reaktionsenthalpie delta H enthält, wird eine thermochemische Gleichung genannt.Betrachten Sie die Verbrennung von Methan eine primäre Brennstoffquelle. Bei der Verbrennung von Methan wird Wärme an die Umgebung abgegeben. Die exotherme Natur der Reaktion wird durch die negative Enthalpieänderung in der thermochemischen Gleichung angezeigt.Die Gleichung für die Verbrennung zeigt dass, wenn 1 Mol Methangas mit 2 Mol Sauerstoffgas reagiert, um 1 Mol Kohlendioxidgas und 2 Mol flüssiges Wasser zu bilden, werden 890, 8 Kilojoule Wärme an die Umgebung abgegeben. Das molare Verhältnis zwischen den Reaktanten oder Produkten und die Reaktionswärme kann als Umrechnungsfaktor verwendet werden, um die während der Reaktion ausgetauschte Wärme zu berechnen. Wenn eine Gasflasche 25, 5 Kilogramm Methan enthält, und das gesamte Methan im Zylinder verbrannt wird, welche Wärmemenge wird erzeugt?Im Allgemeinen, besteht der konzeptionelle Plan darin, die Masse in Mole umzuwandeln und dann Mole in die Reaktionswärme. Zu Beginn werden 25, 5 Kilogramm mit 1000 multipliziert. um die Masse in Gramm zu berechnen.Dann wird die Masse des Methans durch seine molare Masse geteilt 16, 0 Gramm pro Mol, um 1594 Mol Methan zu erhalten. Schließlich benutzt man den Umrechnungsfaktor zwischen Methanmolen und Reaktionswärme, 1594 Mol Methan setzen 14, 2 mal zehn zu den 6 Kilojoule Wärme frei-das ist die Wärme der Reaktion. Die Antwort ist negativ, da die Reaktion exotherm ist, da in der Reaktion Wärme entsteht.

<ol>
	<li>Canagaratna, Sebastian G. "Eine visuelle Hilfe bei Enthalpieberechnungen." Zeitschrift für chemische Bildung 77, Nr. 9 (2000): 1178.</li>
	<li>Keifer, David. "Enthalpie und der zweite Hauptsatz der Thermodynamik." Zeitschrift für chemische Bildung 96, Nr. 7 (2019): 1407-1411.</li>
	<li>Khalil, Mutasim I. "Berechnung der Reaktionsenthalpie durch eine Matrixmethode." Zeitschrift für chemische Bildung 77, Nr. 2 (2000): 185. 
	 </li>
</ol>

thermochemische gleichungen

Bei einer chemischen Reaktion (innerhalb des Systems), die bei konstantem Druck abläuft – wobei die einzige verrichtete Arbeit durch Expansion oder Kontraktion geleistet wird – ist die Reaktionsenthalpie (auch Reaktionswärme genannt, ΔH_rxn) gleich der mit der Umgebung ausgetauschten Wärme (q_p). <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-01.png" style="height: 40px;"> Die Enthalpieänderung ist eine extensive Größe und hängt von der Menge der an der Reaktion beteiligten Reaktanten (oder der Anzahl der Mol der Reaktanten) ab. Die Änderung der Enthalpie ist abhängig von der Reaktion und damit von den physikalischen Zuständen der Reaktanten- und Produktspezies. Eine exotherme Reaktion wird durch einen −ΔH_rxn-Wert beschrieben, während eine endotherme Reaktion einen +ΔH_rxn-Wert besitzt. Da die durch eine Reaktion freigesetzte oder absorbierte Wärmemenge der Menge der durch die Reaktion verbrauchten oder erzeugten Stoffe entspricht, ist es praktisch, eine thermochemische Gleichung zu verwenden, um die Änderungen der Stoffe als auch der Energie darzustellen. In einer thermochemischen Gleichung wird die Änderung der Enthalpie einer Reaktion als ΔH_rxn dargestellt und am Ende der Reaktionsgleichung angegeben. Die Größe von ΔH_rxn gibt die Wärmemenge an, die mit der in der chemischen Gleichung dargestellten Reaktion verbunden ist. Das Vorzeichen von ΔH_rxn gibt an, ob die Reaktion exotherm oder endotherm ist. In der folgenden Gleichung reagieren 1 Mol Wasserstoffgas und 1/2 Mol Sauerstoffgas (bei einer bestimmten Temperatur und einem bestimmten Druck) zu 1 Mol flüssigem Wasser (bei gleicher Temperatur und gleichem Druck). <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-02.png" style="height: 40px;"> Diese Gleichung besagt, dass 286 kJ Wärme an die Umgebung abgegeben werden. Mit anderen Worten: Für jedes verbrauchte Mol Wasserstoff oder für jedes produzierte Mol Wasser werden 286 kJ Wärme freigesetzt (die Reaktion ist exotherm). Daher ist die Reaktionsenthalpie ein Umrechnungsfaktor, der zur Berechnung der Wärmemenge verwendet werden kann, die bei Reaktionen mit bestimmten Mengen an Reaktanten und Produkten freigesetzt oder absorbiert wird. <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-03.png" style="height: 80px;"> Wenn die Koeffizienten der chemischen Gleichung mit einem Faktor multipliziert werden (d. h. wenn sich die Menge eines Stoffes ändert), muss die Änderung der Enthalpie mit demselben Faktor multipliziert werden. (Verdoppelung der Beträge) <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-04.png" style="height: 40px;"> (Verdoppelung der Beträge) <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-05.png" style="height: 40px;"> Um zu veranschaulichen, dass die Enthalpieänderung einer Reaktion von den physikalischen Zuständen der Reaktanten und Produkte abhängt, betrachten wir die Bildung von gasförmigem Wasser (oder Wasserdampf). Wenn 1 Mol Wasserstoffgas und ½ Mol Sauerstoffgas zu 1 Mol gasförmigem Wasser reagieren, werden nur 242 kJ Wärme freigesetzt, im Gegensatz zu 286 kJ Wärme die bei der Bildung von flüssigem Wasser freigesetzt werden. <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/799/799_Equations-06.png" style="height: 40px;">

Thermochemische Gleichungen

Für eine chemische Reaktion (das System), die bei konstantem Druck durchgeführt wird – wobei die einzige Arbeit, die geleistet wird, durch Ausdehnung oder Kontraktion verursacht wird – ...

Education

Lehre

JoVE Core

Chemie

Eins

Thermochemistry

Thermochemie

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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

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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 Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

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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HIgh School

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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Heat Changes in Chemical Equations

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