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Understanding Thermodynamic Changes: Bonds and Entropy

This text explores the principles of thermodynamics, explaining how changes in internal states relate to bonds, entropy, and the mobility of systems. The enthalpy change (ΔH) is influenced by the types and numbers of bonds that are formed and broken during a transition from an initial to a final state. Additionally, the change in entropy (ΔS) is determined by the randomness and the number of accessible iso-energetic states in the system. A higher number of iso-energetic states corresponds to greater entropy, highlighting the relationship between microstates and thermodynamic behavior.

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Understanding Thermodynamic Changes: Bonds and Entropy

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  1. DG = DH -TDS DH depends on the numbers and kinds (covalent and non-covalent) of BONDS made and broken upon going from initial to final state. DS depends on the mobilities and/or randomness (i.e. the number of iso-energetic states) of the system and surroundings upon going from initial to final state. The more isoenergetic states for a system, the greater the entropy of that system.

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