* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download dx cx dx and x - Cameron University
Thermodynamic equilibrium wikipedia , lookup
Detailed balance wikipedia , lookup
Marcus theory wikipedia , lookup
George S. Hammond wikipedia , lookup
State of matter wikipedia , lookup
Determination of equilibrium constants wikipedia , lookup
Statistical mechanics wikipedia , lookup
Physical organic chemistry wikipedia , lookup
Spinodal decomposition wikipedia , lookup
Vapor–liquid equilibrium wikipedia , lookup
Eigenstate thermalization hypothesis wikipedia , lookup
Temperature wikipedia , lookup
Chemical potential wikipedia , lookup
Stability constants of complexes wikipedia , lookup
Van der Waals equation wikipedia , lookup
Heat transfer physics wikipedia , lookup
Transition state theory wikipedia , lookup
Maximum entropy thermodynamics wikipedia , lookup
Equation of state wikipedia , lookup
Chemical equilibrium wikipedia , lookup
Gibbs paradox wikipedia , lookup
Equilibrium chemistry wikipedia , lookup
Work (thermodynamics) wikipedia , lookup
Thermodynamics wikipedia , lookup
CHEM 4353 Learning Objectives Fall 2009 (Buckley) Textbook References are to Physical Chemistry, Ira ,. Levine, 6th Edition, 2009. Objective Textbook Reference Chapter 1- Thermodynamics 1.1 Define and apply the terms system, surroundings, universe, permeable, impermeable, reversible, irreversible, equilibrium, adiabatic, nonadiabatic, extensive properties, intensive properties, open, and closed systems 2.1 Define temperature 2.2 State the Zeroth Law of Thermodynamics 3.1 Work with and interconvert pressure units of pascals, atm, and torr 3.2 State and apply Boyle’s Law 3.3 State and apply Charles’ Law 3.4 State and apply the ideal gas law for pure gas systems 3.5 Treat mixtures of gases using the concept of partial pressure and the ideal gas law 4.1 Evaluate the derivative d/dx of f(x) = ax, f(x) = ln x, and f(x) = axn at least 4.2 Apply the chain rule to differentiate a function 4.3 Given a multiple variable expression, determine the partial derivatives with respect to the variables 4.4 Determine the total differential of a function given sufficient information 5.1 State and apply the van der Waals equation of state 5.2 State the differences at the molecular level between an ideal gas and a van der Waals gas 5.3 Define and apply the terms thermal expansivity and isothermal compressibility 6.1 Evaluate definite integrals such as: ∫ b a cx n dx and ∫ b a dx and others that involve sums x Chapter 2 – The First Law of Thermodynamics 7.1 Define work as the product of a displacement and a force acting in the displacement’s direction 7.2 Identify the work-energy theorem as saying work done by a force on a particle equals the change in kinetic energy of the particle 7.3 Evaluate the work done in various physical situations 7.4 Distinguish between a reversible and irreversible P-V change for a gas 7.5 Evaluate the work done in a reversible isothermal P-V change for an ideal gas 7.6 Evaluate the work done in an irreversible isothermal P-V change for any gas 8.1 Interconvert units of Joules and calories 8.2 Define and apply the concept of specific heat 9.1 State the First Law of Thermodynamics as )U = q + w and state its conditions 9.2 Calculate the change in internal energy in some simple physical processes 10.1 Identify the enthalpy change in a system as the heat flow at constant pressure under certain conditions 10.2 Identify the internal energy change as the heat flow in a constant volume process under certain conditions 1.2 Thermodynamics 1.3 Temperature 1.5 Ideal Gases 1.6 Differential Calculus Chapter 4 (Barrante) 1.7 Equations of State 1.8 Integral Calculus Chapter 5 (Barrante) 2.1 Classical Mechanics 2.2 P-V Work 2.3 Heat 2.4 The First Law of Thermodynamics 2.5 Enthalpy Needs work? Got it? CHEM 4353 Learning Objectives Fall 2009 (Buckley) Textbook References are to Physical Chemistry, Ira ,. Levine, 6th Edition, 2009. Objective Textbook Reference 11.1 Distinguish between the Cv and Cp 11.2 Apply the relationship for a perfect gas the CP,m – CV,m = R 11.2 Define the Joule and Joule-Thomson coefficients 11.3 Apply ∂U ∂H = −Cv µ J and = −CP µ JT given sufficient information ∂V T ∂P T 12.1 Apply heat, work, internal energy and enthalpy concepts to the reversible isothermal P-V change in a perfect gas 12.2 Apply heat, work, internal energy and enthalpy concepts to the reversible constant-P (or constant-V) process in a perfect gas 12.3 Apply heat, work, internal energy and enthalpy concepts to the reversible adiabatic P-V change in a perfect gas 12.4 Apply heat, work, internal energy and enthalpy concepts to a reversible phase change at constant T and P 12.5 Apply heat, work, internal energy and enthalpy concepts to a constant-pressure heating with no phase change 12.6 Apply heat, work, internal energy and enthalpy concepts to a constant-volume heating with no phase change 12.7 Apply heat, work, internal energy and enthalpy concepts to a perfect gas change of state 12.8 Apply heat, work, internal energy and enthalpy concepts to an irreversible adiabatic volume change of a perfect gas 13.1 Distinguish between exact and inexact differentials 13.2 Distinguish between state and path functions in terms of differentials 14.1 Apply the equipartition principle to predict Uv,m, Cv,m, and Cp,m for simple gas phase systems Chapter 3 – The Second Law of Thermodynamics 15.1 Give the Kelvin-Plance statement of the Second Law of Thermodynamics (paraphrase it, at least) 15.2 Give the Clausius statement of the Second Law of Thermodynamics (paraphrase it, at least) 15.3 Given sufficient information, determine the efficiency of a heat engine 15.4 Describe the steps in a Carnot cycle 16.1 State the definition of entropy in terms of dqrev and T 2.6 Heat Capacities 2.7 The Joule and JouleThomson Experiments 2.8 Perfect Gases and the First Law 2.9 Calculation of First Law Quantities 2.10 State Functions and Line Integrals (Barrante) Section 7-7 Exact and Inexact Differentials 2.11 The Molecular Nature of Internal Energy 31. The Second Law of Thermodynamics 3.2 Heat Engines 3.3 Entropy Needs work? Got it? CHEM 4353 Learning Objectives Fall 2009 (Buckley) Textbook References are to Physical Chemistry, Ira ,. Levine, 6th Edition, 2009. Objective Textbook Reference 16.2 Determine the entropy change in a cyclic process ()S = 0, since S is a state function) 16.3 Determine the entropy change in a reversible adiabatic process 16.4 Determine the entropy change in a reversible phase change at constant temperature and pressure 16.5 Determine the entropy change in a reversible isothermal process 16.6 Determine the entropy change in a constant-pressure temperature change with no phase change 16.7 Determine the entropy change in a reversible change of state of a perfect gas 16.8 Determine the entropy change in an irreversible change of state of a perfect gas 16.9 Outline for a physical process viable pathways for computing the entropy changes 16.10 Relate entropy to the reversibility and irreversibility of a process 16.11 Calculate the entropy change in a simple physical process based on a probability function Chapter 4 – Material Equilibrium 17.1 Determine the direction of spontaneity of a process by applying the expression dS ≥ dq when its conditions T are met 17.2 Derive the state function definitions for Gibbs energy and Helmholtz energy from the concepts of internal energy and entropy. 17.3 State the conditions under which the Gibbs energy and the Helmholtz energy indicate spontaneity 18.1 Generate the Gibbs equations based on the definition of U, H, A, and G 18.2 Apply the Euler reciprocity relationship to obtain the Maxwell relations 18.3 Use the Maxwell relations to determine the change in state functions during selected physical changes 19.1 Define the chemical potential 20.1 Explain the role of chemical potential in predicting the direction of phase change 20.2 Given sufficient information, predict the direction of phase change 21.1 Write a chemical equation in mathematical form (Equation 4.94) 21.2 Write the expression for extent of reaction given a chemical equation 21.3 State the condition for equilibrium in a chemical-reaction system in terms of chemical potential Chapter 5 – Standard Thermodynamic Functions of Reactions 3.4 Calculation of Entropy Changes 3.5 Entropy, Reversibility, and Irreversibility 3.7 What is Entropy? 4.2 Entropy and Equilibrium 4.3 The Gibbs and Helmholtz Energies 4.4 Thermodynamic Relations for a System in Equilibrium 4.5 Calculation of Changes in State Functions 4.6 Chemical Potentials and Material Equilibrium 4.7 Phase Equilibrium 4.8 Reaction Equilibrium Needs work? Got it? CHEM 4353 Learning Objectives Fall 2009 (Buckley) Textbook References are to Physical Chemistry, Ira ,. Levine, 6th Edition, 2009. Objective Textbook Reference 22.1 Define the standard state for a pure substance 22.2 22.3 22.4 22.5 22.6 22.7 Define in words the standard enthalpy (change) of reaction, )HET Define in words the standard enthalpy of formation, )fHET Given sufficient information, determine the standard enthalpy change of a reaction from calorimetry Given sufficient information, determine the standard enthalpy change of a reaction from the )fHET Relate )UE to )HE Given sufficient information, determine the standard enthalpy change of a reaction from Hess’s Law 22.8 Given sufficient information, determine the standard enthalpy change for a reaction at different temperatures 22.9 Use Excel to create a polynomial fit to a set of heat capacity data 22.10 Use Excel to create a table indicating the standard enthalpy of reaction for a reaction at different temperatures 23.1 23.2 23.3 24.1 24.2 State the Third Law of Thermodynamics Determine heat capacity of a material at low T using the Debye approach Given sufficient information, calculate the absolute entropy of a material at temperatures above 0 K Use bond additivity to estimate thermodynamic properties Use group additivity to estimate thermodynamic properties Chapter 6 – Reaction Equilibrium in Ideal Gas Mixtures 25.1 Determine the chemical potential of a pure ideal gas (Equation 6.2) 25.2 Determine the chemical potential of a component of an ideal gas mixture (Equation 6.4) 26.1 Relate )GE to KPE 26.2 Interconvert between KPE, KcE, and KxE 26.3 Describe the effects of temperature on equilibria based on )GE = )HE - T)SE 27.1 Apply the van’t Hoff equation to evaluate KPE at different temperatures 28.1 Determine equilibrium concentrations given sufficient information 28.2 Use Excel to solve an equilibrium problem through a numerical approach 29.1 Apply LeChatelier’s Principle to predict the direction of shifts in equilibrium with changing conditions 5.1 Standard States of Pure Substances 5.2 Standard Enthalpy of Reaction 5.3 Standard Enthalpy of Formation 5.4 Determination of Standard Enthalpies of Formation and Reaction 5.5 Temperature Dependence of Reaction Rates 5.6 Use of a Spreadsheet to Obtain a Polynomial Fit 5.7 Conventional Entropies and the Third Law 5.10 Estimation of Thermodynamic Properties 6.1 Chemical Potentials in an Ideal Gas Mixture 6.2 Ideal-Gas Reaction Equilibrium 6.3 Temperature Dependence of the Equilibrium Constant 6.4 Ideal-gas Equilibrium Calculations 6.6 Shifts in Ideal-Gas Reaction Equilibria Needs work? Got it? CHEM 4353 Learning Objectives Fall 2009 (Buckley) Textbook References are to Physical Chemistry, Ira ,. Levine, 6th Edition, 2009. Objective Textbook Reference Chapter 7 – One-Component Phase Equilibrium and Surfaces 30.1 State the phase rule 30.2 Define the terms phase, component, and degree of freedom 30.3 Apply the phase rule to physical systems 31.1 Given sufficient information, construct a one-component phase diagram 31.2 Interpret regions of the one-component phase diagram in terms of the phase rule 32.1 State the Clausius and Clausius-Clapeyron equation and identify the conditions under which the ClausiusClapeyron equation applies 32.2 Apply the Clausius and Clausius-Claperyon equations 33.1 Define a higher-order phase transitions Chapter 8 – Real Gases 34.1 Define the compressibility factor, Z 34.2 Determine the Z for a real gas given its equation of state 35.1 Define the terms critical temperature, critical pressure, critical volume, fluid, and supercritical fluid 36.1 State the Law of Corresponding States 36.2 Use the Law of Corresponding States to predict physical properties of real gases Chapter 9 – Solutions 37.1 Define partial molar volume, partial molar Gibbs energy, partial molar Helmholtz energy, partial molar internal energy, partial molar enthalpy 37.2 Define chemical potential and indicate its significance in terms of evaluating equilibrium 37.3 Given sufficient information determine the partial molar quantities of a substance using the intercept method 38.1 State the molecular-level criteria that lead to an ideal solution 38.2 Determine )mixG, )mixH and )mixS of mixing for an ideal solution 7.1 The Phase Rule 7.2 One-Component Phase Equilibrium 7.3 The Clapeyron Equation 7.5 Higher-Order Phase Transitions 8.1 Compression Factors 8.2 Real-Gas Equations of State 8.3 Condensation 8.7 The Law of Corresponding States 9.2 Partial Molar Quantities 9.4 Determination of Partial Molar Quantities 9.5 Ideal Solutions Needs work? Got it?