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Related Concept Videos

Entropy01:18

Entropy

3.8K
The first law of thermodynamics is quantitatively formulated via an equation relating the internal energy of a system, the heat exchanged by it, and the work done on it. A quantitative formulation of the second law of thermodynamics leads to defining a state function, the entropy.
When an ideal gas expands isothermally, the disorder in the gas increases. From the molecular perspective, the gas molecules have more volume to move around in.
Consider an infinitesimal step in the expansion, which...
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Entropy02:39

Entropy

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Salt particles that have dissolved in water never spontaneously come back together in solution to reform solid particles. Moreover, a gas that has expanded in a vacuum remains dispersed and never spontaneously reassembles. The unidirectional nature of these phenomena is the result of a thermodynamic state function called entropy (S). Entropy is the measure of the extent to which the energy is dispersed throughout a system, or in other words, it is proportional to the degree of disorder of a...
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Enthalpy of Solution02:39

Enthalpy of Solution

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There are two criteria that favor, but do not guarantee, the spontaneous formation of a solution:
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Enthalpy02:59

Enthalpy

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Chemists ordinarily use a property known as enthalpy (H) to describe the thermodynamics of chemical and physical processes. Enthalpy is defined as the sum of a system’s internal energy (E) and the mathematical product of its pressure (P) and volume (V):
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Hess's Law03:40

Hess's Law

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There are two ways to determine the amount of heat involved in a chemical change: measure it experimentally, or calculate it from other experimentally determined enthalpy changes. Some reactions are difficult, if not impossible, to investigate and make accurate measurements for experimentally. And even when a reaction is not hard to perform or measure, it is convenient to be able to determine the heat involved in a reaction without having to perform an experiment.
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Joule-Thomson Effect01:21

Joule-Thomson Effect

11.2K
The Joule-Thomson effect, also known as the Joule-Kelvin effect, describes the temperature change of a fluid when it is forced through a valve or porous plug while keeping it in a thermally insulated environment. This experiment is called a throttling process. This is an important effect widely used in refrigeration and the liquefaction of gases.
This experiment forces high-pressure gas through a throttle valve or a porous plug to a lower-pressure region. The gas expands as it passes through to...
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Related Experiment Video

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Differential Scanning Calorimetry &#8212; A Method for Assessing the Thermal Stability and Conformation of Protein Antigen
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Enthalpy-Entropy Compensation (EEC) Effect: A Revisit.

Animesh Pan1, Tapas Biswas1, Animesh K Rakshit2

  • 1Centre for Surface Science, Department of Chemistry, Jadavpur University , Kolkata 700032, India.

The Journal of Physical Chemistry. B
|December 8, 2015
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Summary
This summary is machine-generated.

This study revisits the fundamentals of iso-kinetic relation (IKR) and enthalpy-entropy compensation (EEC) phenomena. It explores their thermodynamic basis and potential statistical explanations, offering insights into chemical process correlations.

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Area of Science:

  • Physical Chemistry
  • Chemical Thermodynamics
  • Chemical Kinetics

Background:

  • Iso-kinetic relation (IKR) and enthalpy-entropy compensation (EEC) are empirical correlations.
  • While often considered extra-thermodynamic, linear H-S correlations can be thermodynamically deduced.
  • Statistical thermodynamics offers potential explanations for these phenomena.

Purpose of the Study:

  • To revisit the fundamental principles of IKR and EEC from kinetic and thermodynamic perspectives.
  • To provide a detailed examination of the EEC phenomenon across various kinetic and equilibrium processes.
  • To discuss potential correlations between free energy, enthalpy, and entropy changes in chemical processes.

Main Methods:

  • Revisiting fundamental kinetic and thermodynamic principles of IKR and EEC.
  • Detailed analysis of EEC in diverse kinetic and equilibrium systems.
  • Discussion of correlations between thermodynamic parameters (ΔG, ΔH, ΔS) under varied conditions.

Main Results:

  • Clarification of the thermodynamic underpinnings of IKR and EEC.
  • Demonstration of EEC applicability to a range of chemical processes.
  • Exploration of relationships between enthalpy, entropy, and free energy changes.

Conclusions:

  • IKR and EEC phenomena possess both empirical and thermodynamic relevance.
  • Statistical thermodynamics provides a framework for understanding these compensation effects.
  • Further research can explore broader correlations and predictive capabilities for chemical processes.