Final answer:
Thermodynamics properties like Enthalpy, Entropy, and Free Energy can be categorized as extensive or intensive, and each has defining equations or characteristics that can be matched with descriptions given in a Column-II format.
Step-by-step explanation:
In thermodynamics, we distinguish between properties based on how they scale with the amount of matter in the system. Enthalpy (H), Entropy (S), and Free Energy (G) are all crucial concepts in this field. Below, we'll match the thermodynamic properties in Column-I with the corresponding descriptions in Column-II.
- (A) Enthalpy (H) matches with (p) Extensive property. Enthalpy is defined as the sum of the internal energy of a system and the product of its pressure (P) and volume (V), and it is dependent on the amount of substance present.
- (B) Entropy (S) matches with (s) Intensive property. Although in some contexts it can be treated as extensive, typically entropy is considered as an intensive property for a given state, independent of the amount of substance.
- (C) Free energy (G) matches with (q) H - TS. Free energy is defined as the enthalpy of a system minus the product of the temperature (T) and entropy (S), often used to predict the spontaneity of a reaction.
- (D) Pressure matches with (r) E + PV. This does not seem to be a match since pressure is an intensive property, not represented by E+PV. Instead, pressure is not represented by any of the given options (q, r, s) as it is simply an intensive property, not directly related to enthalpy (H), free energy (G), or the combination of them.
Thermodynamic properties are essential for understanding how energy is transferred and transformed in chemical reactions and physical processes. Their categorization as intensive or extensive helps in predicting the behavior of a substance under various conditions.