All of the following are state functions except
Correct answer: C. q
- A. P
- B. V
- C. q
- D. H (enthalpy)
Explanation
A state function is a property of a system that depends only on the current state of the system, not on the path by which the system arrived at that state. In other words, it is independent of the process undergone by the system. Examples of state functions include pressure (P), volume (V), enthalpy (H), internal energy (U), and temperature (T).Heat is not a state function because it depends on the path taken during a process. The amount of heat transferred to or from a system depends on factors such as the specific heat capacity of the substances involved, the temperature difference, and the nature of the process (e.g., reversible or irreversible). Therefore, heat (q) is not a state function.
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About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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