Thermodynamics Laws
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Questions and Answers

Which law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another?

  • Third Law of Thermodynamics
  • First Law of Thermodynamics (correct)
  • Zeroth Law of Thermodynamics
  • Second Law of Thermodynamics
  • What is the change in energy (ΔE) equal to, according to the First Law of Thermodynamics?

  • Q / W
  • W - Q
  • Q + W
  • Q - W (correct)
  • Which type of system does not exchange matter or energy with its surroundings?

  • Open System
  • Closed System
  • Isolated System (correct)
  • Thermodynamic System
  • What is the total energy of a system, including kinetic energy, potential energy, and potential energy associated with the interactions between particles?

    <p>Internal Energy (U)</p> Signup and view all the answers

    Which of the following is a measure of the total energy of a system, including internal energy and the energy associated with the pressure and volume of a system?

    <p>Enthalpy (H)</p> Signup and view all the answers

    What is the change in entropy (ΔS) equal to, according to the Second Law of Thermodynamics?

    <p>ΔQ / T</p> Signup and view all the answers

    Study Notes

    Thermodynamics

    Laws of Thermodynamics

    • Zeroth Law of Thermodynamics: If two systems are in thermal equilibrium with a third system, then they are also in thermal equilibrium with each other.
    • First Law of Thermodynamics: Energy cannot be created or destroyed, only converted from one form to another. ΔE = Q - W, where ΔE is the change in energy, Q is the heat added, and W is the work done.
    • Second Law of Thermodynamics: The total entropy of a closed system always increases over time, except in reversible processes. ΔS = ΔQ / T, where ΔS is the change in entropy, ΔQ is the heat added, and T is the temperature.
    • Third Law of Thermodynamics: As the temperature of a system approaches absolute zero, the entropy of the system approaches a minimum value.

    Thermodynamic Systems

    • Isolated System: A system that does not exchange matter or energy with its surroundings.
    • Closed System: A system that does not exchange matter with its surroundings, but can exchange energy.
    • Open System: A system that can exchange both matter and energy with its surroundings.

    Thermodynamic Properties

    • Internal Energy (U): The total energy of a system, including kinetic energy, potential energy, and potential energy associated with the interactions between particles.
    • Enthalpy (H): A measure of the total energy of a system, including internal energy and the energy associated with the pressure and volume of a system. H = U + PV, where P is the pressure and V is the volume.
    • Entropy (S): A measure of the disorder or randomness of a system.
    • Free Energy (G): A measure of the energy available to do work in a system. G = H - TS, where T is the temperature and S is the entropy.

    Thermodynamic Processes

    • Isothermal Process: A process that occurs at a constant temperature.
    • Adiabatic Process: A process that occurs without the transfer of heat.
    • Isobaric Process: A process that occurs at a constant pressure.
    • Isochoric Process: A process that occurs at a constant volume.

    Laws of Thermodynamics

    • If two systems are in thermal equilibrium with a third system, then they are also in thermal equilibrium with each other (Zeroth Law of Thermodynamics).
    • Energy cannot be created or destroyed, only converted from one form to another, ΔE = Q - W (First Law of Thermodynamics).
    • The total entropy of a closed system always increases over time, except in reversible processes, ΔS = ΔQ / T (Second Law of Thermodynamics).
    • As the temperature of a system approaches absolute zero, the entropy of the system approaches a minimum value (Third Law of Thermodynamics).

    Thermodynamic Systems

    • An isolated system does not exchange matter or energy with its surroundings.
    • A closed system does not exchange matter with its surroundings, but can exchange energy.
    • An open system can exchange both matter and energy with its surroundings.

    Thermodynamic Properties

    • Internal Energy (U) is the total energy of a system, including kinetic energy, potential energy, and potential energy associated with interactions between particles.
    • Enthalpy (H) is a measure of the total energy of a system, including internal energy and the energy associated with pressure and volume, H = U + PV.
    • Entropy (S) is a measure of the disorder or randomness of a system.
    • Free Energy (G) is a measure of the energy available to do work in a system, G = H - TS.

    Thermodynamic Processes

    • Isothermal Process: a process that occurs at a constant temperature.
    • Adiabatic Process: a process that occurs without the transfer of heat.
    • Isobaric Process: a process that occurs at a constant pressure.
    • Isochoric Process: a process that occurs at a constant volume.

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    Description

    Understand the fundamental principles of thermodynamics, including the zeroth, first, and second laws that govern energy and entropy.

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