Name: using standard enthalpy values in chemistry
Uploaded: 2020-09-03T13:38:27.000Z
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Standard Enthalpy of Formation

반응의 엔탈피 변화는 열량계를 이용하여 측정하거나 반응물과 생성물 간의 엔탈피 차이를 계산하여 구할 수 있습니다. 그러나 반응물 및 생성물의 절대 엔탈피는 직접 측정할 수 없습니다. 따라서 화학자들은 일반적으로 약속된 표준 상태의 기준 물질에 상대적인 엔탈피의 변화 또는 델타 H를 사용합니다.

표준 상태는 조건의 특정 기준에 의해 정의됩니다. 여기에는 일반적으로 섭씨 25도 또는 298 켈빈으로 설정된 온도와 기체의 경우 1 bar의 일정 압력이 포함됩니다. 용액의 경우 표준 상태는 용매 내 순수 용질의 1 몰농도입니다.

물질의 표준 상태는 또한 이러한 조건 하에서 물질이 존재하는 물리적 상태를 포함합니다. 예를 들어, 염화나트륨은 고체이고, 수은은 액체, 헬륨은 기체 상태입니다. 이러한 조건에서 원소가 둘 이상의 형태로 존재하는 경우 원소의 가장 안정적인 형태가 표준 상태로 정의됩니다.

예를 들어 탄소는 흑연 결정체나 다이아몬드로 존재할 수 있지만 흑연이 가장 안정된 형태이며 따라서 탄소의 표준 상태입니다. 표준 상태에 있는 원소들이 결합하여 순수한 화합물 1 몰을 형성할 때 반응의 엔탈피를 표준 생성 엔탈피 또는 표준 생성열이라고 합니다. 이 값은 델타 H 제로, 첨자 f로 표시됩니다.

여기서 제로는 구성 성분의 표준 상태를 나타내고 f는 생성을 나타냅니다. 표준 상태 조건 하에서 순수 원소에 대한 표준 생성 엔탈피는 반응이 없기 때문에 항상 0이며, 따라서 원소가 이미 표준 상태에 있을 때 엔탈피의 변화는 없습니다. 화합물에 대하여 몰당 킬로줄 단위의 표준 생성 엔탈피 값은 참조 표에서 확인할 수 있습니다.

이러한 물질들에는 기체 상태의 나트륨과 같은 비표준 상태의 원소와 염화 나트륨과 같은 화합물이 포함됩니다. 반응의 표준 엔탈피 변화는 생성물과 반응물의 차이에서 계산할 수 있으며, 또는 기준 표의 엔탈피 값을 사용하여 계산할 수 있습니다.

<ol>
	<li>호크, 에릭 리. "알칸 형성의 표준 엔탈피 계산 : 분자 역학 및 스프레드 시트 프로그램 설명." 화학 교육 저널 76, no. 2 (1999) : 278.</li>
	<li>마주카, 제임스 W., 알렉시스 R. 다우닝, 크리스토퍼 포터. "연소 물리 화학 실험실의 엔탈피에 적용된 경험적으로 수정된 전자 구조 계산." 화학 교육 저널 96, no. 6 (2019): 1165-1170.</li>
	<li>Jansen, Michael P. "가솔린 차량을 프로판으로 전환하는 비용. A Practical Review Problem for Senior High School or Introductory Chemistry(고등학교 또는 화학 입문용 실기 복습 문제)."Journal of Chemical Education 77, no. 12 (2000): 1578. 
	 </li>
</ol>

표준 생성 엔탈피

엔탈피 변화는 일반적으로 반응물과 생성물이 모두 동일한 조건에 있는 반응에 대해 표로 작성됩니다. 표준 상태는 다른 다양한 조건에서 특성을 결정하기 위한 기준점으로 사용되는 일반적으로 허용되는 조건 집합입니다. 화학자의 경우 IUPAC 표준 상태는 1bar의 압력과 1M의 용액을 의미하며 온도를 지정하지 않습니다. 많은 열화학 표에는 표준 상태 1atm의 값이 나열되어 있습니다. 반응의 ΔH는 압력의 작은 변화(1bar = 0.987atm)로 거의 변하지 않기 때문에 ΔH 값(가장 정확하게 측정된 값 제외)은 두 표준 조건 세트에서 본질적으로 동일합니다. 엔탈피 변화 기호의 위 첨자 "o"는 표준 상태를 나타냅니다. 일반적인(그러나 기술적으로 표준은 아님) 온도는 298.15K이므로 다른 온도가 지정되지 않는 한 이 온도가 가정됩니다. 따라서 기호(ΔH°)는 이러한 조건에서 발생하는 프로세스의 엔탈피 변화를 나타내는 데 사용됩니다. (기호 ΔH는 비표준 조건에서 발생하는 반응의 엔탈피 변화를 나타내는 데 사용됩니다.)

연소 반응, 상전이 및 형성 반응을 포함한 다양한 유형의 화학적 및 물리적 공정에 대한 엔탈피 변화는 참고 문헌에서 확인할 수 있습니다. 주어진 반응에 대한 엔탈피 변화는 관련된 물질의 양에 비례하기 때문에 이를 기준으로 보고할 수 있습니다(즉, 특정 반응물의 양에 대한 ΔH로). 그러나 우리는 하나의 광범위한 특성(ΔH)을 다른 특성(물질의 양)으로 나누고, 양당 강도 값인 ΔH를 보고하는 것이 더 유용하다는 사실을 종종 발견합니다. 이는 종종 몰당 기준으로 "정규화"됩니다.

표준 생성 엔탈피

표준 생성 엔탈피 ΔH_f°는 표준 상태 조건에서 가장 안정한 상태의 자유 원소로부터 정확히 1몰의 순수 물질이 형성되는 반응에 대한 엔탈피 변화입니다. 이러한 값은 실행하기 어렵거나 위험한 화학 반응에 대한 엔탈피 변화를 계산하거나 예측하는 데 또는 측정하기 어려운 프로세스에 특히 유용합니다. 알려진 표준 생성 엔탈피 값을 사용하여 모든 반응에 대한 엔탈피 변화를 결정할 수 있습니다.

CO_2의 표준 생성 엔탈피(g)는 −393.5 kJ/mol입니다. 발열 반응의 엔탈피 변화는 다음과 같습니다.

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/801/801_Equations-01.png" style="height: 40px;" />

반응물들이 1atm 및 25°C(이 조건에서 가장 안정한 형태인 흑연 상태의 탄소)에서 시작하여 1atm 및 25°C의 1몰의 CO_2로 끝납니다. 이산화질소인 NO_2(g)의 경우 ΔH_f°는 33.2kJ/mol입니다. 흡열 반응의 엔탈피 변화는 다음과 같습니다.

<img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/801/801_Equations-02.png" style="height: 40px;" />

이 경우 표준 생성 엔탈피는 항상 생성물 1몰(NO_2(g))을 참조하기 때문에 ^1/_2몰의 N_2와 1몰의 O_2를 사용한 반응식이 정확합니다.

정의에 따르면, 가장 안정적인 형태의 원소 형성의 표준 엔탈피는 표준 조건에서 0과 같습니다. 예를 들어 탄소(그래핀), 이원자 산소 가스, 이원자 질소 가스, 나트륨 금속 및 액체 수은의 표준 형성 엔탈피는 표준 조건에서 0입니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/5-3-enthalpy">Openstax, Chemistry 2e, Section 5.3: Enthalpy.</a>

엔탈피 변화는 일반적으로 반응물과 생성물이 모두 동일한 조건에 있는 반응에 대해 표로 작성됩니다. 표준 상태는 일반적으로 ...

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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 | JoVE K12

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Use mathematics and computational thinking to execute simple calorimetric calculations based on the Law of Conservation of Energy.

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Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

gas-laws-boyle-s-gay-lussac-charles-avogadro-s-and-ideal-gas-law

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

chemical-stoichiometry-gases-using-ideal-gas-law-to-determine

Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

In addition to measuring quantities ...

basic-postulates-kinetic-molecular-theory-particle-size-energy

Basic Postulates of Kinetic Molecular Theory: Particle Size, Energy, and Collision

The ideal-gas equation, which is empirical, describes the behavior of gases by establishing relationships between their macroscopic properties. For ...

kinetic-molecular-theory-gas-laws-explain-properties-gas

Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws ...

kinetic-molecular-theory-molecular-velocities-temperature-kinetic

Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

The kinetic molecular theory qualitatively explains the behaviors described by the various gas laws. The postulates of this theory may be applied in a ...

behavior-gas-molecules-molecular-diffusion-mean-free-path

Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many ...

real-gases-effects-intermolecular-forces-molecular-volume-deriving

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and ...

Ideal Gas Law

Source: Laboratory of Dr. Andreas Z&#252;ttel - Swiss Federal Laboratories for Materials Science and Technology
The ideal gas law describes the behavior ...

Derivation of the Ideal Gas Law
Gases are a fundamental state of matter. A gas is a collection of molecules that have a significant distance between their ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
	According to the ideal gas law for a given ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

PS.Chm.7.3

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

Using Standard Enthalpy Values in Chemistry

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