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Read Alberty's publication (Pure Appl. Chem., Vol.73, No. 8, pp. 1349-1380, 2001) on Legendre Transforms of U. Generate all the Legendre functions from the relation U = U(S, V, n) of an open one-phase system and the associated Maxwell relations

Read Alberty's publication (Pure Appl. Chem., Vol.73, No. 8, pp. 1349-1380, 2001) on Legendre Transforms of U. Generate all the Legendre functions from the relation U = U(S, V, n) of an open one-phase system and the associated Maxwell relations

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ACTIVITY 2-4 part 2. Answer only no. 2

This is sometimes called the heat content at constant pressure process, qp . Activity 2-4 Let us make use of our knowledge of calculus and derive some thermodynamic relationships from certain functions. 1. Internal energy's natural variables are entropy, S, and V. Mathematically, it can be written as U = U(S,V). Write the total differential of U. Derive the Maxwell relation from the total differential and evaluate the partial differentials. 2. Read Alberty's publication (Pure Appl. Chem., Vol.73, No. 8, pp. 1349-1380, 2001) on Legendre Transforms of U. Generate all the Legendre functions from the relation U = U(S, V, n) of an open one-phase system and the associated Maxwell relations
Transcribed Image Text:This is sometimes called the heat content at constant pressure process, qp . Activity 2-4 Let us make use of our knowledge of calculus and derive some thermodynamic relationships from certain functions. 1. Internal energy's natural variables are entropy, S, and V. Mathematically, it can be written as U = U(S,V). Write the total differential of U. Derive the Maxwell relation from the total differential and evaluate the partial differentials. 2. Read Alberty's publication (Pure Appl. Chem., Vol.73, No. 8, pp. 1349-1380, 2001) on Legendre Transforms of U. Generate all the Legendre functions from the relation U = U(S, V, n) of an open one-phase system and the associated Maxwell relations
2.2. The First Law of Thermodynamics [ “YOU CAN’T WIN"] The first law of thermvdynamies relates the change in internal energy as the system changes state. Internal energy, U, represents the total energy of the system which is given as the sum of the kinetie and potential energy of the molecules in the system. Since the absolute value of internal energy cannot be measured, only changes in internal energy (AU) are measureable as systems change from one state to another state. The change in internal energy is measured at constant volume processes. Thus it is sometimes referred to as the heat content at constant volume, q, . The first law is often called as the Law of Conservation of Energy which states that energy cannot be created or destroyed; it can only be transformed from one form into another. The basic energy currency in the first law is heat and work. The mathematical statement of the law is AU = q + w du = đq + đw or where q is positive when it is absorbed by the system and negative when heat is released into the surrounding. In pressure-volume (PV) work, w is defined as w = - Pop dV, where pop is the opposing or external pressure Work is positive when the surrounding does work on the system; it is negative when the system does work on the surrounding. The first law can be stated in this mann er - the change in internal energy of the system is equal to the sum of the heat absorbed by the system plus the work done on the system by the surrounding. Vision: The premier untversity of science and technology in the Visayas Mission: Provide excellent instruction, conduct relevant research and faster community engagement that produce highly competent graduates for the development of the country Page 40 Chem 150 Physical Chemistry Learning Resource Internal energy, U, is a state function. Changes in its value depends only on the internal energies of the final and initial states, e.g., AU = Uánal - Umitial - However, q and w are path functions. Their magnitudes depend on how the change in state is achieved. This entails different ways of solving for the q and w depending on the change of state processes involved. The change in enthalpy, AH, unlike AU, is measured at constant pressure. This is sometimes ealled the heat content at constant pressure process, qp -
Transcribed Image Text:2.2. The First Law of Thermodynamics [ “YOU CAN’T WIN"] The first law of thermvdynamies relates the change in internal energy as the system changes state. Internal energy, U, represents the total energy of the system which is given as the sum of the kinetie and potential energy of the molecules in the system. Since the absolute value of internal energy cannot be measured, only changes in internal energy (AU) are measureable as systems change from one state to another state. The change in internal energy is measured at constant volume processes. Thus it is sometimes referred to as the heat content at constant volume, q, . The first law is often called as the Law of Conservation of Energy which states that energy cannot be created or destroyed; it can only be transformed from one form into another. The basic energy currency in the first law is heat and work. The mathematical statement of the law is AU = q + w du = đq + đw or where q is positive when it is absorbed by the system and negative when heat is released into the surrounding. In pressure-volume (PV) work, w is defined as w = - Pop dV, where pop is the opposing or external pressure Work is positive when the surrounding does work on the system; it is negative when the system does work on the surrounding. The first law can be stated in this mann er - the change in internal energy of the system is equal to the sum of the heat absorbed by the system plus the work done on the system by the surrounding. Vision: The premier untversity of science and technology in the Visayas Mission: Provide excellent instruction, conduct relevant research and faster community engagement that produce highly competent graduates for the development of the country Page 40 Chem 150 Physical Chemistry Learning Resource Internal energy, U, is a state function. Changes in its value depends only on the internal energies of the final and initial states, e.g., AU = Uánal - Umitial - However, q and w are path functions. Their magnitudes depend on how the change in state is achieved. This entails different ways of solving for the q and w depending on the change of state processes involved. The change in enthalpy, AH, unlike AU, is measured at constant pressure. This is sometimes ealled the heat content at constant pressure process, qp -
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