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Exploring the fundamental thermodynamic relation, this overview highlights the role of entropy in chemical thermodynamics, its significance in open systems, and its impact on phase transitions. It delves into entropy generation, changes in ideal gas processes, and the thermodynamics of phase changes, providing essential insights into the behavior of systems under various conditions.
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The fundamental thermodynamic relation is an essential equation in thermodynamics that describes the internal energy change of a system
This relation is applicable to any process, including those that are not quasistatic, meaning the system may not be in equilibrium during the transition
It forms the basis for deriving other important thermodynamic equations, such as the Maxwell relations and the equations for heat capacities, which are applicable to all systems irrespective of their microscopic details
Entropy is a fundamental concept in chemical thermodynamics, representing the degree of disorder or randomness in a system
According to the second law of thermodynamics, the total entropy of an isolated system can never decrease over time, and it is at a maximum at equilibrium
The Clausius definition of entropy allows for the calculation of entropy change (ΔS) through the equation δq_rev/T = ΔS
Open systems, which exchange mass and energy with their surroundings, are common in chemical engineering and are analyzed using the principles of thermodynamics
The entropy balance for an open system is given by dS/dt = Σ(Ṁ_kŜ_k) + (Q̇/T) + Ŝ_gen
Entropy generation occurs due to irreversible processes such as chemical reactions, heat transfer, and friction, and is always non-negative, consistent with the second law of thermodynamics
The entropy change in ideal gas processes can be quantified using specific equations
For an isothermal process, where the temperature remains constant, the change in entropy (ΔS) is given by ΔS = nR ln(V/V_0) for volume changes, or ΔS = -nR ln(P/P_0) for pressure changes
For processes at constant volume or pressure, the entropy change is related to the heat capacity, with ΔS = nC_P ln(T/T_0) for constant pressure and ΔS = nC_v ln(T/T_0) for constant volume
00
The equation representing this concept is written as dU = TdS - pdV, where dU signifies the ______ change in internal energy.
differential
01
In the equation dU = TdS - pdV, T stands for the ______ temperature and dS for the differential change in ______.
absolute
entropy
02
The variable 'p' in the fundamental thermodynamic relation denotes ______, while dV represents the differential change in ______.
pressure
volume
