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11.1: Internal Energy

  • Page ID
    238253
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    The internal energy of a system is identified with the random, disordered motion of molecules; the total (internal) energy in a system includes potential and kinetic energy. This is contrast to external energy which is a function of the sample with respect to the outside environment (e.g. kinetic energy if the sample is moving or potential energy if the sample is at a height from the ground etc). The symbol for Internal Energy Change is \( ΔU\).

    Energy on a smaller scale

    • Internal energy includes energy on a microscopic scale
    • It is the sum of all the microscopic energies such as:
      1. translational kinetic energy
      2. vibrational and rotational kinetic energy
      3. potential energy from intermolecular forces
    Example

    One gram of water at zero °Celsius compared with one gram of copper at zero °Celsius do NOT have the same internal energy because even though their kinetic energies are equal, water has a much higher potential energy causing its internal energy to be much greater than the copper's internal energy.

    Internal Energy Change Equations

    The first law of thermodynamics states:

    \[dU=dq+dw\]

    where \(dq\) is heat and \(dw\) is work.

    An isolated system cannot exchange heat or work with its surroundings making the change in internal energy equal to zero:

    \[dU_{\text {isolated system}} = 0\]

    Therefore, in an isolated system:

    \[dq=-dw\]

    Energy is Conserved

    Ryan's chem wiki.jpg

    \[dU_{\text {isolated system}} = dU_{\text {system}} + dU_{\text {surroundings}}\]

    \[dU_{\text {system}}= -dU_{\text {surroundings}}\]

    The signs of internal energy

    • Energy entering the system is POSITIVE (+), meaning heat is absorbed, q>0. Work is thus done on the system, w>0
    • Energy leaving the system is NEGATIVE (-), meaning heat is given off by the system, q<0 and work is done by the system, w<0

    Quick Notes

    • A system contains ONLY Internal Energy
    • A system does NOT contain energy in the form of heat or work
    • Heat and work only exist during a change in the system; they are path functions
    • Internal energy is a state function

    Outside Links

    • Levine, Ira N. "Thermodynamic internal energy of an ideal gas of rigid rotors." J. Chem. Educ. 1985: 62, 53.

    Contributors

    • Lorraine Alborzfar (UCD)

    11.1: Internal Energy is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.