What does the equation ∆G = ∆H - T∆S represent?

The equation ∆G = ∆H - T∆S describes the relationship between the change in Gibbs free energy (∆G), the change in enthalpy (∆H), and the change in entropy (∆S) of a system at a given temperature (T). This equation is fundamental in thermodynamics, particularly in predicting the spontaneity of a chemical reaction.

Gibbs free energy (∆G) is a crucial parameter that indicates whether a process or reaction can occur spontaneously. A negative value of ∆G suggests that the reaction is spontaneous under the given conditions, while a positive value indicates non-spontaneity. The term ∆H represents the heat content or enthalpy change of the system, which reflects the energy absorbed or released during the reaction. The term T∆S accounts for the effect of entropy, which is a measure of the disorder or randomness in the system.

By using this relationship, one can determine the conditions under which a reaction will be spontaneous. It highlights the interplay between energy (enthalpy) and disorder (entropy), emphasizing that a reaction's spontaneity is influenced by both thermodynamic parameters and temperature.

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