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Internal Energy

    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.

    1. 1. Energy on a smaller scale
    2. 2. Internal Energy Change Equations
    3. 3. Quick Notes
    4. 4. Outside Links
    5. 5. Contributors

    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

    ΔU = q+w

    where q is heat and w is work

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

    ΔUisolated system = 0

    Energy is Conserved

    Ryan's chem wiki.jpg

    ΔUsystem = -ΔUsurroundings

    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
    • Since ΔUisolated system = 0, ΔUsystem = -ΔUsurroundings and energy is conserved.

    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
    • Internal energy is a state function

    Contributors

    • Lorraine Alborzfar (UCD)

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