Please note that the content of this book primarily consists of articles available from Wikipedia or other free sources online. When a chemical reaction exhibits a linear relationship between enthalpy and entropy, one might observe what is known as an Enthalpy-Entropy Compensation, where the magnitude of change in the Gibbs free energy is less than one might expect. Mathematically, this is because of the Gibbs free energy equation ( G = H – T S), where the change in enthalpy ( H) and the change in entropy ( S) have opposite signs— G will change very little if both enthalpy and entropy increase. For instance, in a reaction where the chemical bonds become stronger or where chemical bonds are being formed throughout the course of a reaction a negative H value will result. At the same time, this aforementioned act of forming or even strengthening a bond will limit the movement of the molecule (in terms of the molecule’s ability to rotate, vibrate, etc.) and hence decrease the molecule’s entropy. This leads to a fairly small G value. This effect is frequently invoked in the discussion of the thermodynamics of proteins, ligands, and nucleic acids.

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