Is entropy only defined for constant temperature andtemperature enthalpy and entropy state functions and are S and Delta S functions of temperature?
The constant temperature because entropy can change with temperature. Furthermore, since S is a state function, we do not need to specify whether this process is reversible or irreversible. State functions are those values which depend only on the state of the system and not on how it is reached e.g., enthalpy, entropy, temperature and free energy. Path functions are those values which depend on the path of the system. Is a function of temperature but Deltas is not a function of temperature.
Entropy (S) is defined for a system at any given temperature. It is a state function and does not depend on the path taken to reach that state. The concept of entropy applies to systems at both constant temperature and varying temperature conditions.
Enthalpy (H) is also a state function and is defined for a system at a specific temperature. It represents the heat content of a system and is related to the internal energy (U) of the system.
Both entropy and enthalpy are functions of temperature. As the temperature changes, the values of entropy and enthalpy can vary. The dependence of entropy and enthalpy on temperature is typically expressed through their temperature coefficients or derivatives.
Delta entropy (ΔS) represents the change in entropy between two states of a system undergoing a process. It is also a state function and can be calculated as the difference between the entropy of the final state (S_final) and the entropy of the initial state (S_initial): ΔS = S_final - S_initial. The change in entropy can be influenced by changes in temperature, as well as other factors such as phase transitions or chemical reactions.
In summary, entropy and enthalpy are state functions and are dependent on temperature. Delta entropy (ΔS) represents the change in entropy between two states, and its value can be influenced by changes in temperature and other factors.
The entropy of a substance increases with its molecular weight and complexity and with temperature. The entropy also increases as the pressure or concentration becomes smaller. Entropies of gases are much larger than those of condensed phases. This is only defined for constant temperature because entropy can change with temperature. Furthermore, since S is a state function, we do not need to specify whether this process is reversible or irreversible. The conditions in terms of entropy and temperature of an endothermic reaction to be spontaneous. Enthalpy typically rises in endothermic processes. Yet, when the enthalpy and entropy changes result in a negative Gibbs free energy, an endothermic process may happen on its own. Internal energy, enthalpy, and entropy are examples of state quantities or state functions because they quantitatively describe an equilibrium state of a thermodynamic system, regardless of how the system has arrived in that state. (a) ΔS are a state function. (b) If a system undergoes a reversible change, the entropy of the universe increases. (c) If a system undergoes a reversible process, the change in entropy of the system is exactly matched by an equal and opposite. Change in the entropy of the surroundings. Heat (q) and work (w) are path functions, not state functions: They are path dependent. They are energy transfer → they are not intrinsic to the system. The symbol for entropy is S, and a change in entropy is shown as “delta” S or ΔS. If the entropy of a system increases, ΔS are positive. If the entropy of a system decreases, ΔS are negative.
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