If we consider a hot object in a cold room as our complete system, then the thermal energy in our system is not very well dispersed because it’s more concentrated in the hot object. For example, we know that higher temperature means a greater average thermal energy per molecule, so we can think of temperature as a measure of the concentration of thermal energy in an object. By isolated system we mean one for which energy does not leave or enter. In order to aid in our study of other thermodynamic processes, such as phase changes, a more general version of the Second Law can be stated in terms of energy concentration and dispersion: a ny spontaneous process must move an isolated system toward a state of more uniform dispersion of energy throughout the system. The Second Law of Thermodynamics introduced in the previous chapters states that thermal energy will always spontaneously transfer from higher temperature to lower temperature.
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