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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
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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
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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
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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
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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
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