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Related Concept Videos

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Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to...
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When a substance—isolated from its environment—is subjected to heat changes, corresponding changes in temperature and phase of the substance is observed; this is graphically represented by heating and cooling curves.
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The thermodynamic processes can be classified into reversible and irreversible processes. The processes that can be restored to their initial state are called reversible processes. It is only possible if the process is in quasi-static equilibrium, i.e., it takes place in infinitesimally small steps, and the system remains at equilibrium However, these are ideal processes and do not occur naturally. An ideal system undergoing a reversible process is always in thermodynamic equilibrium within...
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Phase Transitions: Melting and Freezing02:39

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Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
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The internal energy of a substance—the total kinetic energy of all its molecules and the potential energy of their associated forces—depends on the strength of the intermolecular forces in the condensed phases and the pressure exerted on the substance. The internal energy of a substance is the highest in the gaseous state, the lowest in the solid state, and intermediate in the liquid state. Phase transitions are caused by changes in physical conditions, such as temperature and...
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Converting work to heat is an irreversible process, and the purpose of a heat engine is to reverse the effect partially. Heat engines aim to increase the efficiency of the reversal, that is, maximize the work retrieved from heat. If the efficiency of a heat engine were 100%, it would imply reversing the process completely without introducing any other effect. Thus, it would violate the second law of thermodynamics.
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Author Spotlight: Simulation and Analysis of the Temperature Rise of Ring Main Unit Equipment
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Continuous nonequilibrium transition driven by heat flow.

Yirui Zhang1, Marek Litniewski1, Karol Makuch1

  • 1Institute of Physical Chemistry, Polish Academy of Sciences, Kasprzaka 44/52, PL-01-224 Warsaw, Poland.

Physical Review. E
|September 16, 2021
PubMed
Summary
This summary is machine-generated.

Researchers found a new out-of-equilibrium transition in gases. At critical heat flux, the gas separates into hot, low-density, and cold, dense regions, demonstrating a novel thermodynamic state.

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Area of Science:

  • Thermodynamics
  • Statistical Mechanics
  • Non-equilibrium Physics

Background:

  • Understanding non-equilibrium systems is crucial for many physical phenomena.
  • Characterizing phase transitions in systems driven out-of-equilibrium remains a challenge.

Purpose of the Study:

  • To discover and characterize an out-of-equilibrium phase transition in an ideal gas system.
  • To explore the thermodynamic principles governing such transitions.

Main Methods:

  • Theoretical analysis of an ideal gas confined between two walls with a movable adiabatic partition.
  • Driving the system out-of-equilibrium by direct energy supply into the gas volume.
  • Molecular dynamic simulations using a soft-sphere fluid model to validate findings in an interacting system.

Main Results:

  • Identified a continuous, out-of-equilibrium transition at a critical heat flux.
  • Observed gas separation into distinct hot, low-density and cold, dense regions.
  • Confirmed the transition's existence in both ideal and interacting gas systems via simulations.

Conclusions:

  • The discovered transition serves as a paradigm for understanding stationary states in non-equilibrium systems.
  • Introduced a stationary state Helmholtz-like function for thermodynamic description of these states.
  • The findings offer new insights into the behavior of matter under continuous energy flux.