Name: using standard enthalpy values in chemistry
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PS.Chm.7.2

Standard Enthalpy of Formation

Bir reaksiyonun entalpi değişimi, kalorimetre kullanılarak ölçülebilir veya reaktanlar ve ürünler arasındaki entalpi farkı hesaplanarak bulunabilir. Bununla birlikte, reaktanların ve ürünlerin mutlak entalpileri doğrudan ölçülemez;bu nedenle, kimyagerler genellikle üzerinde mutabık kalınan standart bir durumda bir referans maddeye göre entalpi veya delta H'deki değişimi kullanırlar. Standart durum, belirli bir dizi koşulla tanımlanır.Bu, genellikle 25 Santigrat derece veya 298 Kelvin olmak üzere sabit bir sıcaklığı ve gazlar için 1 bar sabit basıncı içerir. Çözeltiler için standart hal, bir çözücü içinde saf bir çözünen maddenin 1 molar konsantrasyonudur. Bir maddenin standart hali, maddenin bu koşullar altında içinde bulunduğu fiziksel durumu da içerir.Örneğin katı olarak sodyum klorür, sıvı olarak cıva veya gaz olarak Helyum. Bu koşullar altında bir element birden fazla formda mevcutsa, elementin en kararlı formu standart hal olarak tanımlanır. Örneğin karbon, grafit kristalleri veya elmas olarak var olabilir, ancak grafit en kararlı formudur ve bu nedenle, karbonun standart halidir.Standart hallerindeki elementler, 1 mol saf bileşik oluşturmak için birleştiğinde, Reaksiyon entalpisine standart entalpi veya standart oluşum ısısı denir. Bu, delta H sıfır, alt simge f ile gösterilir, burada sıfır, kurucu elementlerin standart hallerini belirtirken, f oluşumu gösterir. Standart hal koşulları altında saf elementler için standart oluşum entalpisi her zaman sıfırdır, çünkü reaksiyon yoktur ve bu nedenle element zaten standart haldeyken entalpide değişiklik olmaz.Bir bileşiğin mol başına kilojul cinsinden standart oluşum entalpisinin değerleri, referans tablolarında bulunabilir. Bu maddeler, gaz halindeki sodyum gibi standart olmayan hallerdeki elementleri ve sodyum klorür gibi bileşikleri içerir. Bir reaksiyonun standart entalpi değişimi, ürün ve reaktan farkından hesaplanabilir ve bu da referans tablodaki entalpi değerleri kullanılarak hesaplanabilir.

<ol>
	<li>Şahin, Eric Leigh. "Alkan oluşumunun standart entalpilerinin hesaplanması: Moleküler mekanik ve elektronik tablo programlarının gösterilmesi." Kimya eğitimi dergisi 76, no. 2 (1999): 278.</li>
	<li>Mazzuca, James W., Alexis R. Downing ve Christopher Potter. "Yanma entalpisine uygulanan ampirik olarak düzeltilmiş elektronik yapı hesaplamaları fiziksel kimya laboratuvarı." Kimya Eğitimi Dergisi 96, no. 6 (2019): 1165-1170.</li>
	<li>Jansen, Michael P. "Benzinle çalışan bir aracı propana dönüştürmenin maliyeti. Lise Sonu veya Kimyaya Giriş için Pratik Bir İnceleme Problemi." Kimya Eğitimi Dergisi 77, no. 12 (2000): 1578. 
	 </li>
</ol>

standart oluşum entalpisi

Entalpi değişiklikleri tipik olarak hem reaktanların hem de ürünlerin aynı koşullarda olduğu reaksiyonlar için tablo halinde verilmiştir. Standart bir durum, diğer farklı koşullar altında özelliklerin belirlenmesi için bir referans noktası olarak kullanılan, yaygın olarak kabul edilen bir dizi koşuldur. Kimyacılar için IUPAC standart durumu, 1 bar basınç altındaki malzemeleri ve 1 M'deki çözeltileri ifade eder ve bir sıcaklık belirtmez. Çoğu termokimyasal tablo, 1 atm standart durumdaki değerleri listeler. Bir reaksiyonun ΔH'si basınçtaki bu kadar küçük değişikliklerle (1 bar = 0,987 atm) çok az değiştiğinden, ΔH değerleri (en hassas şekilde ölçülen değerler hariç), her iki standart koşul setinde de temelde aynıdır. Entalpi değişim sembolündeki üst simge “o”, standart durumu belirtir. Normal (ancak teknik olarak standart olmayan) sıcaklık 298,15 K olduğundan, başka bir sıcaklık belirtilmedikçe bu sıcaklık varsayılacaktır. Bu nedenle, (ΔH°) sembolü, bu koşullar altında meydana gelen bir süreç için entalpi değişikliğini belirtmek için kullanılır. (ΔH sembolü, standart olmayan koşullar altında meydana gelen bir reaksiyon için bir entalpi değişikliğini belirtmek için kullanılır.)
 
 Yanma reaksiyonları, faz geçişleri ve oluşum reaksiyonları dahil olmak üzere birçok kimyasal ve fiziksel süreç için entalpi değişiklikleri referans literatürde mevcuttur. Belirli bir reaksiyon için entalpi değişikliği, ilgili maddelerin miktarlarıyla orantılı olduğundan, bu temelde rapor edilebilir (yani, belirli miktarlarda reaktanlar için ΔH olarak). Bununla birlikte, genellikle bir kapsamlı özelliği (ΔH) diğerine (madde miktarı) bölmek ve genellikle mol başına “normalize” edilmiş ΔH miktar başına yoğun bir değeri raporlamayı daha yararlı buluyoruz. 
 
 <h4>Standart Oluşum Entalpisi</h4>
 
 Standart oluşum entalpisi ΔHf°, standart durum koşulları altında en kararlı hallerinde serbest elementlerden tam olarak 1 mol saf maddenin oluştuğu bir reaksiyon için entalpi değişimidir. Bu değerler, gerçekleştirilmesi pratik olmayan veya tehlikeli olan kimyasal reaksiyonlar için veya ölçüm yapmanın zor olduğu süreçler için entalpi değişikliklerini hesaplamak veya tahmin etmek için özellikle yararlıdır. Standart oluşum entalpilerinin bilinen değerleri kullanılarak, herhangi bir reaksiyon için entalpi değişimi belirlenebilir.
 
 Standart CO2 (g) oluşum entalpisi −393,5 kJ/mol'dür. Bu, ekzotermik reaksiyon için entalpi değişimidir: 
 
 <img alt=""Eq1"" src=""https://www.jovecore.com/CDNSource/lessons/801/801_Equations-01.png"" style=""height: 40px;"" />
 
 1 atm ve 25 °C'lik bir basınçta reaktanlarla başlayarak (karbonun grafit olarak mevcut olması, bu koşullar altında karbonun en kararlı formu) ve yine 1 atm ve 25 °C'de 1 mol CO2 ile bitmektedir. Nitrojen dioksit için NO2 (g), ΔHf° 33,2 kJ/mol'dür. Bu, endotermik reaksiyon için entalpi değişimidir:
 
 <img alt=""Eq2"" src=""https://www.jovecore.com/CDNSource/lessons/801/801_Equations-02.png"" style=""height: 40px;"" />
 
 1/2 mol N2 ve 1 mol O2 içeren bir reaksiyon denklemi bu durumda doğrudur çünkü standart oluşum entalpisi her zaman 1 mol ürünü ifade eder: NO2 (g).
 
 Tanım olarak, bir elementin en kararlı formundaki standart oluşum entalpisi, standart koşullar altında sıfıra eşittir. Örneğin, standart koşullar altında karbon (grafen), diatomik oksijen gazı, diatomik nitrojen gazı, sodyum metali ve sıvı cıva oluşumunun standart entalpileri sıfırdır.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy"">Openstax, Chemistry 2e, Section 5.3: Enthalpy.</a>

Standart Oluşum Entalpisi

Entalpi değişiklikleri tipik olarak hem reaktanların hem de ürünlerin aynı koşullarda olduğu reaksiyonlar için tablo haline getirilir. Standart bir durum yaygın olarak ...

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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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