What Is Enthalpy: Definition, Importance And Applications!

Enthalpy; Definition, Importance And Applications: This article will talk about Enthalpy and its definition, importance and applications. Students can get a basic understanding of Enthalpy.

Jul 8, 2024, 17:43 IST
What Is Enthalpy: Definition, Importance And Applications!
What Is Enthalpy: Definition, Importance And Applications!

Enthalpy; Definition, Importance And Applications: Enthalpy is the measurement of energy in a thermodynamic system. It is a fundamental concept in thermodynamics. It represents the total energy content of a system, considering both its internal energy and energy associated with its volume and pressure. 

Here’s a breakdown of Enthalpy: 

  • Internal Energy (u)- This refers to the inherent energy of the particles within the system, like the kinetic energy from their motion and the potential energy being stored in chemical bonds. 
  • Pressure-Volume Work (PV)- Imagine a system expanding against a constant external pressure. This work requires energy and PV captures the energy distribution. So the formula becomes: 
  • Enthalpy is mathematically defined as the sum of these two components: H=U+PV

Why Is Enthalpy Important? 

Enthalpy is useful as it simplifies the calculation of processes happening at a constant pressure, which is often the case in chemistry labs or natural processes occurring at atmospheric pressure. 

  • Exothermic Vs. Endothermic Reactions: Chemical reactions can release heat or absorb heat. The sign of ΔH can tell you this. A positive ΔH indicates an endothermic reaction while a negative. One indicates an exothermic reaction. 
  • Phase Transitions: Enthalpy changes are associated with phase transitions like melting, vaporization, and sublimation. 

The change in Enthalpy can be shown as: 

ΔH=ΔU+ΔPV

If the pressure and temperature don’t change throughout the process, and the task is limited to pressure and volume, then the change in enthalpy is given by: 

ΔH=ΔU+PΔV

The flow of the heat q at a constant pressure in the process is equal to the change in enthalpy based on the following equation.

ΔH=q

A relationship between q and ΔH can be defined if q is endothermic or exothermic. An endothermic reaction absorbs heat and reveals that heat is consumed in the form of a reaction from the surroundings. As q>0, if q is positive, then ΔH is also positive. If the heat is released as an exothermic reaction, the heat is given to the surroundings. So, if q<0, then  ΔH will be negative if q is negative.

Applications Of Enthalpy

Chemical Reactions: Enthalpy change is the fundamental property used to classify chemical reactions as exothermic or endothermic. This knowledge is crucial in designing and optimising the chemical processes for industrial applications. 

Designing Materials: Enthalpy changes are considered during material selection and design. Understanding the enthalpy of fusion is crucial in metallurgy to determine the amount of heat required to melt a metal for casting. 

Biological Processes: Even many biological systems utilise enthalpy. 

With the help of these notes, students can get detailed information on the concept of enthalpy and can study easily. 

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Akshita Jolly
Akshita Jolly

Content Writer

Akshita Jolly is a multimedia professional specialising in education, entertainment, fashion, health, and lifestyle news. Holding a degree in Journalism and Mass Communication, she has contributed to renowned media organisations, including the Press Trust of India. She currently serves as Executive – Editorial at Jagran New Media, where she writes, edits, and manages content for the School and News sections of the Jagran Josh (English) portal. She also creates engaging and informative videos for the Jagran Josh YouTube platform, helping to make educational content more accessible and dynamic. Her work has contributed to reaching over 10 million monthly users, reflecting both the impact and scale of her content. For inquiries, she can be reached at akshitajolly@jagrannewmedia.com.
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