Name: using standard enthalpy values in chemistry
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Standard Enthalpy of Formation

Die Enthalpieänderung einer Reaktion kann mit einem Kalorimeter gemessen werden, oder es kann berechnet werden durch den Enthalpieunterschied zwischen den Reaktanten und den Produkten. Die absoluten Enthalpien der Reaktanten und Produkten können nicht direkt gemessen werden;daher, verwenden Chemiker im Allgemeinen die Änderung der Enthalpie oder Delta H, relativ zu einer Referenzsubstanz in einem definiertem Standardzustand. Der Standardzustand wird durch einen bestimmten Satz von Bedingungen definiert.Dazu gehört eine bestimmte Temperatur, normalerweise 25 Grad Celsius oder 298 Kelvin, und ein konstanter Druck von 1 bar für Gase. Für Lösungen ist der Standardzustand eine 1-molare Konzentration eines reinen gelösten Stoffes in einem Lösungsmittel. Der Standardzustand für einen Stoff umfasst auch den physikalischen Zustand der Materie in dem der Stoff unter diesen Bedingungen existiert.Zum Beispiel Natriumchlorid als Feststoff, Quecksilber als Flüssigkeit, oder Helium als Gas. Wenn ein Element in mehr als einer Form unter diesen Bedingungen existiert, ist die stabilste Form des Elements als sein Standardzustand definiert. Zum Beispiel kann Kohlenstoff in Form von Graphitkristallen oder als Diamant vorliegen, aber Graphit ist die stabilste Form und damit den Standardzustand von Kohlenstoff.Wenn Elemente in ihren Standardzuständen miteinander reagieren um 1 Mol einer reinen Verbindung zu bilden, wird die Enthalpie der Reaktion die Standardenthalpie, oder Standardwärme der Bildung bezeichnet. Dies wird mit delta H null bezeichnet, tiefgestellt f, wobei null die Standardzustände der teilnehmenden Elemente angibt, während f die Bildung anzeigt. Die Standardbildungsenthalpie für reine Elemente unter Standardzustandsbedingungen ist immer Null, weil es keine Reaktion gibt, und daher keine Änderung der Enthalpie, wenn das Element bereits in seinem Standardzustand ist.Die Werte der Standardenthalpie der Bildung in Kilojoule pro Mol für eine Verbindung sind in Referenztabellen zu finden. Diese Substanzen umfassen Elemente in nicht standardisierten Zuständen, wie z. B.gasförmiges Natrium, und Verbindungen wie Natriumchlorid.Die Standard-Enthalpieänderung einer Reaktion kann aus der Differenz der Produkte und Reaktanten berechnet werden, die ihrerseits unter Verwendung der Enthalpiewerte aus der Referenztabelle berechnet werden.

<ol>
	<li>Falke, Eric Leigh. "Die Berechnung von Standardenthalpien der Bildung von Alkanen: Veranschaulichung der Molekularmechanik und Tabellenkalkulationsprogramme." Zeitschrift für chemische Bildung 76, Nr. 2 (1999): 278.</li>
	<li>Mazzuca, James W., Alexis R. Downing und Christopher Potter. "Empirisch korrigierte elektronische Strukturberechnungen, die auf das Labor für physikalische Chemie der Verbrennungsenthalpie angewendet werden." Zeitschrift für chemische Bildung 96, Nr. 6 (2019): 1165-1170.</li>
	<li>Jansen, Michael P. "Die Kosten für die Umrüstung eines benzinbetriebenen Fahrzeugs auf Propan. Ein praktisches Wiederholungsproblem für die Oberstufe oder die Einführung in die Chemie." Zeitschrift für chemische Bildung 77, Nr. 12 (2000): 1578. 
	 </li>
</ol>

standardbildungsenthalpie

Enthalpieänderungen für Reaktionen werden typischerweise tabellarisch aufgeführt, bei denen sowohl die Reaktanten als auch die Produkte die gleichen Bedingungen aufweisen. Ein Standardzustand ist ein allgemein akzeptierter Satz von Bedingungen, der als Referenzpunkt für die Bestimmung von Eigenschaften unter anderen unterschiedlichen Bedingungen dient. Für Chemiker bezieht sich der IUPAC-Standardzustand auf Materialien unter einem Druck von 1 bar und Lösungen bei 1 M und gibt keine Temperatur an. In vielen thermochemischen Tabellen sind Werte mit einem Standardzustand von 1 atm aufgeführt. Da sich das ΔH einer Reaktion bei so kleinen Druckänderungen (1 bar = 0,987 atm) nur sehr wenig ändert, sind die ΔH-Werte (mit Ausnahme der genauesten Messwerte) unter beiden Standardbedingungen im Wesentlichen gleich. Ein hochgestelltes „o“ im Enthalpieänderungssymbol bezeichnet den Standardzustand. Da die übliche (aber technisch nicht genormte) Temperatur 298,15 K beträgt, wird diese Temperatur angenommen, sofern keine andere Temperatur angegeben ist. Daher wird das Symbol (ΔH°) verwendet, um eine Enthalpieänderung für einen Prozess anzuzeigen, der unter diesen Bedingungen auftritt. (Das Symbol ΔH wird verwendet, um eine Enthalpieänderung für eine Reaktion anzuzeigen, die unter nicht standardmäßigen Bedingungen abläuft.) Die Enthalpieänderungen für viele Arten chemischer und physikalischer Prozesse sind in der Referenzliteratur verfügbar, einschließlich derjenigen für Verbrennungsreaktionen, Phasenübergänge und Bildungsreaktionen. Da die Enthalpieänderung für eine bestimmte Reaktion proportional zu den beteiligten Stoffmengen ist, kann sie auf dieser Grundlage angegeben werden (d. h. als ΔH für bestimmte Mengen an Reaktanten). Wir finden es jedoch häufig nützlicher, eine umfangreiche Eigenschaft (ΔH) durch eine andere (Substanzmenge) zu dividieren und einen intensiven Wert von ΔH pro Menge anzugeben, der häufig auf die Basis pro Mol „normiert“ wird. <h4>Standardbildungsenthalpie</h4> Die Standardbildungsenthalpie ΔHf° ist eine Enthalpieänderung für eine Reaktion, bei der genau 1 Mol einer reinen Substanz aus freien Elementen in ihren stabilsten Zuständen unter Standardzustandsbedingungen gebildet wird. Diese Werte sind besonders nützlich für die Berechnung oder Vorhersage von Enthalpieänderungen bei chemischen Reaktionen, deren Durchführung unpraktisch oder gefährlich ist, oder für Prozesse, für die es schwierig ist, Messungen durchzuführen. Unter Verwendung bekannter Werte der Standardbildungsenthalpien kann die Enthalpieänderung für jede Reaktion bestimmt werden. Die Standardbildungsenthalpie von CO2 (g) beträgt −393,5 kJ/mol. Dies ist die Enthalpieänderung für die exotherme Reaktion: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/801/801_Equations-01.png" style="height: 40px;"> Beginnend mit den Reaktanten bei einem Druck von 1 atm und 25 °C (wobei der Kohlenstoff als Graphit vorliegt, die unter diesen Bedingungen stabilste Form von Kohlenstoff) und endend mit einem Mol CO2, ebenfalls bei 1 atm und 25 °C. Für Stickstoffdioxid, NO2 (g), beträgt ΔHf° 33,2 kJ/mol. Dies ist die Enthalpieänderung für die endotherme Reaktion: <img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/801/801_Equations-02.png" style="height: 40px;"> Eine Reaktionsgleichung mit 1/2 Mol N2 und 1 Mol O2 ist in diesem Fall korrekt, da sich die Standardbildungsenthalpie immer auf 1 Mol Produkt bezieht: NO2 (g). Per Definition ist die Standardbildungsenthalpie eines Elements in seiner stabilsten Form unter Standardbedingungen gleich Null. Beispielsweise sind die Standardbildungsenthalpien von Kohlenstoff (Graphen), zweiatomigem Sauerstoffgas, zweiatomigem Stickstoffgas, Natriummetall und flüssigem Quecksilber unter Standardbedingungen Null. Dieser Text wurde angepasst von <a href="https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy">Openstax, Chemistry 2e, Section 5.3: Enthalpy.</a>

Standardbildungsenthalpie

Enthalpieänderungen werden typischerweise für Reaktionen tabellarisch dargestellt, bei denen sowohl die Reaktanten als auch die Produkte die gleichen Bedingungen aufweisen. Ein Standardzustand ist in der Regel ein ...

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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 the enthalpy symbol shows that the value is for standard state. The usual temperature is 298.15 K, so ΔH° is often used for a process under these conditions. ΔH is used for nonstandard conditions.

Standard enthalpy values are available for many chemical and physical processes. These include combustion reactions, phase changes, and formation reactions. Enthalpy change depends on the amount of substance involved, so it can be reported for a specific reaction amount. It is often more useful to divide by moles and give a per-mole value.

The standard enthalpy of formation, ΔHf°, is the enthalpy change when 1 mole of a pure substance forms from its elements in their most stable states under standard conditions. This value is useful when a reaction is hard to measure directly or would be unsafe to run. Known formation enthalpies can also be used to calculate the enthalpy change of other reactions.

For example, the standard enthalpy of formation of CO2(g) is −393.5 kJ/mol. That value matches the exothermic formation of one mole of carbon dioxide from graphite, the most stable form of carbon under these conditions, with all substances at 1 atm and 25 °C. For NO2(g), ΔHf° is 33.2 kJ/mol. Here the balanced formation reaction uses 1/2 mole of N2 and 1 mole of O2 because the value must refer to 1 mole of NO2 product.

By definition, an element in its most stable form has a standard enthalpy of formation of zero. Examples include carbon as graphene, diatomic oxygen gas, diatomic nitrogen gas, sodium metal, and liquid mercury. These zero values help make thermochemical calculations consistent.

Using Standard Enthalpy Values in Chemistry

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Using Standard Enthalpy Values in Chemistry

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