thermodynamic

(adjective)

Relating to the conversion of heat into other forms of energy.

Related Terms

  • intermolecular
  • plasma

Examples of thermodynamic in the following topics:

  • The Zeroth Law of Thermodynamics

    • The Zeroth Law of Thermodynamics states that systems in thermal equilibrium are at the same temperature.
    • There are a few ways to state the Zeroth Law of Thermodynamics, but the simplest is as follows: systems that are in thermal equilibrium exist at the same temperature.
    • What the Zeroth Law of Thermodynamics means is that temperature is something worth measuring, because it indicates whether heat will move between objects.
    • However, according to the Zeroth Law of Thermodynamics, if the systems are in thermal equilibrium, no heat flow will take place.
    • There are more formal ways to state the Zeroth Law of Thermodynamics, which is commonly stated in the following manner:
  • A Review of the Zeroth Law

    • Zeroth law justifies the use of thermodynamic temperature, defined as the shared temperature of three designated systems at equilibrium.
    • This law was postulated in the 1930s, after the first and second laws of thermodynamics had been developed and named.
    • This conclusion may seem obvious, because all three have the same temperature, but zeroth law is basic to thermodynamics.
    • A brief introduction to the zeroth and 1st laws of thermodynamics as well as PV diagrams for students.
    • Discuss how the Zeroth Law of Thermodynamics justifies the use of thermodynamic temperature
  • The First Law of Thermodynamics

    • The first law of thermodynamics states that energy can be transferred or transformed, but cannot be created or destroyed.
    • The first law of thermodynamics deals with the total amount of energy in the universe.
    • Thermodynamics often divides the universe into two categories: the system and its surroundings.
    • Another useful form of the first law of thermodynamics relates heat and work for the change in energy of the internal system:
    • A basic diagram showing the fundamental distinction between the system and its surroundings in thermodynamics.
  • The Second Law

    • The second law of thermodynamics states that heat transfer occurs spontaneously only from higher to lower temperature bodies.
    • The second law of thermodynamics deals with the direction taken by spontaneous processes.
    • The law that forbids these processes is called the second law of thermodynamics .
    • A brief introduction to heat engines and thermodynamic concepts such as the Carnot Engine for students.
    • Contrast the concept of irreversibility between the First and Second Laws of Thermodynamics
  • The First Law

    • The 1st law of thermodynamics states that internal energy change of a system equals net heat transfer minus net work done by the system.
    • The first law of thermodynamics is a version of the law of conservation of energy specialized for thermodynamic systems.
    • In equation form, the first law of thermodynamics is
    • In this video I continue with my series of tutorial videos on Thermal Physics and Thermodynamics.
    • Explain how the net heat transferred and net work done in a system relate to the first law of thermodynamics
  • The Three Laws of Thermodynamics

    • The laws of thermodynamics define fundamental physical quantities (temperature, energy, and entropy) that characterize thermodynamic systems.
    • In order to avoid confusion, scientists discuss thermodynamic values in reference to a system and its surroundings.
    • The first law of thermodynamics, also known as Law of Conservation of Energy, states that energy can neither be created nor destroyed; energy can only be transferred or changed from one form to another.
    • The second law of thermodynamics says that the entropy of any isolated system always increases.
    • The third law of thermodynamics states that the entropy of a system approaches a constant value as the temperature approaches absolute zero.
  • Comparison of Enthalpy to Internal Energy

    • Internal energy and enthalpy are both measurements that quantify the amount of energy present in a thermodynamic system.
    • A thermodynamic system can be any physical system with a well-defined volume in space.
    • In thermodynamics, the total energy contained by a given thermodynamic system is referred to the internal energy (U).
    • From a thermodynamic perspective, work can be done on or by the system; similarly, heat can be lost or gained by a particular system.
    • Because the internal energy encompasses only the energy contained within a thermodynamic system, the internal energy of isolated systems cannot change.
  • LTE

    • An extremely useful assumption is that the matter is in thermal equilibrium at least locally (Local Thermodynamic Equilibrium).
    • In this case the ratio of the number of atoms in the various states is determined by the condition of thermodynamic equilibrium
    • Because the source function equals the blackbody function, does this mean that sources in local thermodynamic equilibrium emit blackbody radiation?
  • Thermodynamics of Redox Reactions

    • The thermodynamics of redox reactions can be determined using their standard reduction potentials and the Nernst equation.
    • In order to calculate thermodynamic quantities like change in Gibbs free energy $\Delta G$ for a general redox reaction, an equation called the Nernst equation must be used.
  • Changes in Energy

    • In classical thermodynamics the entropy is interpreted as a state function of a thermodynamic system.
    • The entropy of a system is defined only if it is in thermodynamic equilibrium.
    • In a thermodynamic system, pressure, density, and temperature tend to become uniform over time because this equilibrium state has a higher probability (more possible combinations of microstates) than any other.
    • The entropy of the thermodynamic system is a measure of how far the equalization has progressed.
    • The second law of thermodynamics shows that in an isolated system internal portions at different temperatures will tend to adjust to a single uniform temperature and thus produce equilibrium.
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