All of the following are state functions EXCEPT?
Correct answer: D. q
- A. E
- B. G
- C. H
- D. q
Explanation
Option D, q (heat), is correct because it is not a state function.A state function is a property that depends only on the current state of the system, meaning it doesn't matter how the system reached that state. In contrast, q (heat) is not a state function because the amount of heat exchanged during a process depends on the specific path taken by the system, not just its initial and final states.Options A, B, and C (E, G, and H) are all state functions:- E represents the internal energy of a system.- G represents the Gibbs free energy, which is a measure of the maximum reversible work that can be performed by a system at constant temperature and pressure.- H represents the enthalpy, which is a measure of the heat content of a system at constant pressure.These properties depend only on the initial and final states of the system, making them state functions.
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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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