1
Chapter Objectives for Thermodynamics
Mathematics
Concepts
Know the distinction between an ordinary derivative and a partial derivative.
Know how to take the partial derivative of a function.
Know how to find the partial derivative of a function using the technique of implicit
differentiation.
Know the interchangeability of mixed derivatives.
Know how to invert a partial derivative.
Know how to apply the chain rule to a partial derivative
Understand the distinction between the chain rule and Euler’s chain rule.
Know the applicability of Euler’s chain rule.
Understand the distinction between a derivative and a differential.
Know how to find the total differential of a function.
Know how to test a differential for exactness.
Understand how state functions are related to exact differentials.
Know how to perform a line integral.
Know how to approximate a function using a Taylor series.
Know how to use a Taylor series to fit data to curve.
Know how to use dimensional analysis to check expressional for dimensional consistency.
Terms and Definitions
Partial differentiation
Implicit differentiation
Euler’s chain rule
Differential
Derivative
Total differential
Key Equations
First-tier
 2z   2z 



 xy   yx 
Exact differential
State function
Line integral
Taylor series
Maclaurin series
 M  x, y    N  x, y  

 

y

 x  x
y
 z   z   w 
  

 
 y  x  w  x  y  x
 x   z   y 
       1
 y  z  x  y  z  x
 z 
1
   y
 y  x  
 
 z  x
 M  x, y    N  x, y  

 

y

 x  x
y
 R 
 R 
 R 
 R 
dR  
d  
d  
d
 d  



  , ,
   ,,
  , ,
  ,,
n
1  f  x0 
n
f x  
 x  x0 
n
x
n  0 n!

2
Introduction to Thermodynamics
Concepts
Be able to make the distinction between intensive and extensive thermodynamic quantities.
Know the difference between the thermodynamic control and the kinetic control of a process.
Know how to change the following systems in to each other: open, closed, isolated, adiabatic.
Know the zeroth law of thermodynamics.
Understand the consequences of the zeroth law of thermodynamics.
Be able to compare and contrast the different temperature scales.
Understand the necessity for absolute temperature scales.
Understand how physical properties are used to measure temperature.
Understand the theoretical basis behind the ideal gas thermometer.
Know the fundamental definition for pressure.
Know the distinction between the pressure units, bars and atmospheres.
Be able to make conversions between different pressure units.
Know the theoretical basis of the mercury barometer.
Know how to use open-end and closed-end manometers.
Know how Avogadro’s number is determined with x-ray diffraction data of a crystalline solid.
Terms and Definitions
Intensive
Extensive
Open
Closed
Isolated
Adiabatic
Ideal gas thermometer
Pascal
Bar
Atmosphere(unit)
Barometer
Open-end manometer
Closed-end manometer
Avogadro’s number
Key Equations
First-tier
K.E.  T 
1
mv 2
2
w   Fdl
F = ma
Second-tier
V  V0 1  
T  lim 273.15
p 0
V
Vt.p.
Fx  
V
x
 V    Fx dx
3
Gases
Concepts
Know the basic assumptions of the kinetic theory of gases
Understand the essentials of the argument of how to apply the kinetic theory of gases to calculate
the pressure of a gas
Know the relationship between the ideal gas constant and Boltzmann’s constant and under what
conditions each is used
Know how the root-mean-squared speed of an ensemble of gas molecules is calculated
Understand how a one-dimensional velocity distribution is different than a three-dimensional
velocity distribution
Know how to calculate the average speed, most probable speed and RMS speed of an ensemble
of gas molecules from the Maxwell-Boltzmann distribution function
Be able to sketch the isotherm of an ideal gas on a p-V diagram
Understand Boyle’s law at the molecular level
Be able to sketch the isobar of an ideal gas on a V-T diagram
Understand Charles’ law at the molecular level
Understand Avogadro’s law at the molecular level
Know the proportional relationships between pressure, volume, amount and temperature
Be able to sketch the isochore of an ideal gas on a p-T diagram
Understand how a thermodynamic system can be described using an equation of state
Know how an ideal gas can be defined with microscopic assumptions, a macroscopic definition
or an equation of state
Know how equations of state can be written in terms of the molar volume
Understand how real gases are described with different equations of state
Understand the molecular interpretations of the “a” and “b” parameters in the van der Waals
equation
Know the two different ways that the virial equation of state can be written
Know why a virial equation of state would be used in state of closed equation of state
Understand the significance of the Boyle temperature for a real gas
Know the shape of an isotherm for a real gas above, below and at its critical temperature
Know the slope and curvature of an isotherm at the critical point is zero
From a plot of compressibility versus pressure, know how to interpret microscopically deviations
of compressibility from zero
Know the process for converting a two-parameter closed equation of state into its reduced form
Understand how the law of corresponding states is relating the nonideality of real gas to its
critical point
4
Terms and Definitions
Dalton’s law of partial pressure
Boltzmann constant
Probability density
Maxwell-Boltzmann distribution
Average speed
Most probable speed
Root-mean-squared speed
Barometric distribution law
Boyle’s law
Isotherm
Isothermal compressibility
Charles’ law
Isobar
Avogadro’s law
Isochore
Equation of state
Covolume
van der Waals equation
Virial equation of state
Boyle temperature
Critical point
Compressibility
Reduced variables
Law of corresponding states
Key Equations
First-tier
1
1
 tr  m  v 2x  v 2y  v z2   mv 2
2
2
Fz 
dp z
 ma z
dt
1
vrms

Z
 N vi2  2
  
 i N
v
1  V 


V  p T,n
2

F
A
 tr 
3
kT
2

v   v G  v  dv
  v G  v  dv
2
0
p1V1  p2 V2
0
 U 

 0
 V T
V1 V2

n1 n 2
V1 V2

T1 T2
p
p
RT
a
 2
Vb V
PV
RT
Second-tier
pz  2mvz
2E tr
p
3V
p
p z,i   Fz,i dt  Fz,i
1
2
 3kT   3RT 
v 
 

 m   M 
1
2
RT  B  T  C  T  D  T 



1 
V 
V
V2
V3
Vc  3b
Tc 
8a
27Rb
pc 
a
27b 2
 t 2  t1 
p  p0e
W
z,i
F

  Fz,i 
m vz,i
2
lz
Mgz
RT

RT
1  B  T  p  C  T  p2  D  T  p3 
 p
V


5
The First Law of Thermodynamics
Concepts
Know why the existence of state functions are crucial for the study of thermodynamics
Know why thermodynamic quantities are state function and which are not
Know why the reversibility condition is important for thermodynamic studies
Know why the chemist’s definition of work, w    p ex  dV , is the same as the physicist’s
definition of work w   F  d l
Know the sign convention for work and heat
Understand the microscopic interpretation of work and heat
Understand why the first law of thermodynamics is a statement of the conservation of energy
Know why making the distinction between exact and inexact differentials is important
Understand why chemists will prefer using enthalpy over internal energy to calculate energy
changes
Know how to change a differential relationship (such as the definition of heat capacity) into an
integral relationship
Know how find a partial derivative from the total differential of a function
Understand why Cp is greater than Cv.
Be comfortable using molar quantities (such as molar volume) rather than the extensive
quantities
Know how to calculate isobaric, isochoric, isothermal and adiabatic heat
Know why using the definition for the extant of reaction is help in studying the thermodynamics
of chemical reactions
Know the definitions for the standard state pressure, temperature and concentration
Know the definition of the biological standard state
Know the conceptual basis for Hess’ law
Know how to use Hess’ law to find the enthalpy (or other state function) for a chemical reaction
Know the conceptual basis for using the “products minus reactants” of formation enthalpies to
find the enthalpy of reaction
Be able to compare and contrast constant-pressure calorimetry with constant-volume calorimetry
Know the products of combustion for an organic molecule
Know the general process for measuring the heat of combustion using a bomb calorimeter
Know how to use the enthalpy of combustion of a substance to find its enthalpy of formation
Know how to convert an internal energy change to an enthalpy change and vice versa for a gasphase chemical reaction
Know how to use heat capacity data to calculate energy changes at nonstandard temperatures
Know how to use bond enthalpies to approximate the reaction enthalpy for a chemical reaction
Know why the use bond enthalpies can only give approximate reaction enthalpies
Be able to calculate work under isobaric, isochoric, isothermal and adiabatic conditions
Understand the subtleties distinguishing the Joule coefficient and Joule-Thomson coefficient
Understand how the Joule-Thomson coefficient is measured classically and presently
Understand the significance of the Joule-Thomson coefficient for refrigeration
Be able to calculate internal energy changes for isobaric, isochoric, isothermal and adiabatic
conditions
Be able to calculate enthalpy changes for isobaric, isochoric, isothermal and adiabatic conditions
6
Know the definitions for the six measureable partial derivatives to this point in the class
Know that the internal energy can be considered to be a function of temperature and volume
Know that the enthalpy can be considered to be a function of temperature and pressure
Terms and Definitions
State function
Reversibility
Theorem of maximum work
Work
Heat
Thermal expansivity
Enthalpy
Specific heat
Heat capacity
Extant of reaction
Formation reaction
Bomb calorimeter
Kirchoff’s law
Joule coefficient
Joule-Thomson coefficient
Key Equations
First-tier
p = pex
w    p ex  dV
U  q v
H  q p
 T 
J  

 V U
U  q  w
q  mCT
dU  đq + đw
 H 
Cp  

 T p

 U 
Cv  

 T v
1  V 


V  T p

H = U + PV
n i  n i,0
i
 T 
 JT   
 p H
Second-tier
 U   U   U   V 

 
 
 

 T p  T V  V T  T p
 1  U 

Cp  CV  nR  
  1
 p  V T 
Cp  CV  R
7
The Second Law of Thermodynamics
Concepts
Understand Kelvin’s statement of the 2nd law that no cyclic process can completely convert heat
to work
Understand Clausius’ statement of the 2nd law that no cyclic process can completely heat and
cool without the use of some work
Understand the 2nd law in terms of the entropy of the universe always increasing for any
spontaneous process
Understand how the relationship between volume and temperature is derived for an adiabatic
process
Be able to sketch an isotherm and adiabat on a p-V diagram to distinguish between the two
process
Know the thermodynamic definition of entropy
Be able to sketch a Carnot cycle on a p-V diagram
Know how the Carnot cycle is used to proof that entropy is state function
How the change of entropy of an ideal gas in the Carnot cycle is zero
How the change of entropy for any substance in the Carnot cycle is zero
How the change of entropy for any substance in any cycle is zero
Know why the efficiency of a heat engine approaches 100% only if it is cooled to absolute zero
Understand the statistical view of entropy especially in terms of dispersal of energy states
Know how to calculate the entropy change of a substance for given change of temperature
Know how to calculate the entropy change of a phase transition
Understand why standard state entropies are not zero (in contrast to standard state enthalpies)
Know how to calculate the standard entropy change of a reaction from a stoichiometric sum of
standard entropies
Understand why Trouton’s rule is approximately valid
Be able to make a precise statement of the third law of thermodynamics
Know the Nernst heat theorem
Understand the consequences of the third law of thermodynamics
Know the application of the Einstein-Debye law
Understand how to calculate a standard state entropy
Understand the derivation of the equation dA  0 for constant temperature and volume conditions
Understand the derivation of the equation dG  0 for constant temperature and pressure conditions
Understand how free energy predicts the spontaneity of physical or chemical process
Know that the value of free energy yields the maximum amount of available work for a process
Know how to find the Gibbsian relationships from the differential of internal energy, enthalpy,
Helmholtz free energy and Gibbs free energy
Understand conceptually the origin of the Gibbsian relationships
Know how to find the Maxwell relationships from the differential of internal energy, enthalpy,
Helmholtz free energy and Gibbs free energy
Understand conceptually the origin of the Maxwell relationships
Understand the relationship between fugacity and pressure
Know how a thermodynamic equilibrium constant is defined in terms of fugacities
Understand conceptually how fugacity coefficients can be found from experimental
compressibility data
Know the derivation for the pressure dependence of Gibbs free energy
8
Know how the coefficient of performance for a refrigerator is related to the efficiency of a heat
engine
Know the power requirement for refrigeration grow quadratically with cooling requirement
Know that the performance of a refrigerator decreases as temperature decreases
Understand the basic processes behind adiabatic demagnetization when it is used to ultralow
temperatures
Understand how evaporative cooling works
Understand how a heat pump is similar to an air conditioner
Terms and Definitions
Spontaneous process
Heat capacity ratio
Adiabat
Carnot cycle
Efficiency
Trouton’s rule
Nernst heat theorem
Einstein-Debye law
Helmholtz free energy
Gibbs free energy
Maxwell’s relations
Fugacity
Thermodynamic equilibrium constant
Fugacity coefficient
Gibbs-Helmholtz equation
Coefficient of performance
Adiabatic Demagnetization
Heat pump
Key Equations
First-tier
dq
dS  rev
T
Sf
 dS 
Si
Tf

Ti

Cp dT
T
dU  T dS  p dV
Cp
Cv

1

2
p1V  p 2 V
Srxn   iSi0
w

qh
A = U – TS
dH  T dS  V dp
Tf
Si
Ti
 dS  
Cv dT
T
G = H – TS
dA  p dV  SdT
 U 

  p
 V S
 H 

 T
 S p
 A 

  p
 V T
 A 

  S
 T V
 G 

 V
 p T
H
   G
 2
 
T
 T p T
R  Nk
Sf
i
 U 

 T
 S V
 T 
 p 

   
 V S
 S V
T
  1 c
Th
 T 
 V 
   

 S p
 p S
f p
dG  SdT  V dp
 H 

 V
 p S
 G 

  S
 T  p
 p 
 S 
  

 T V  V T
p 
G f  Gi  nRT ln  f 
 pi 
c
qc
w
 S 
 V 

   
 T p
 p T
f
K
f
p0   f D p0 
c
C
p0   f B p0 
a
A
d
b
9
Second-tier
T2  V1 
 
T1  V2 
1
qh qc

Th Tc
S  k ln 
V 
S  nR ln  f 
 Vi 

C v  aT 3
f
i
 Z 1 

 dp  ln 
 p 
Chemical Equilibrium
Concepts
Know the definition of chemical potential as partial molar Gibbs free energy
Be able to rewrite the differentials of internal energy, enthalpy, Helmholtz free energy and Gibbs
free energy to the functional dependence of the amount of substance
Know how to derive the pressure dependence of the chemical potential for a gas
Understand how the definition of the reaction quotient (and equilibrium constant) arises from the
Gibbs free energy of reaction
Understand the difference between the Gibbs free energy of reaction and the standard Gibbs free
energy of reaction
Know how the definition of the reaction quotient is affected for heterogeneous equilibria
Understand the meaning of the van’t Hoff equation in its integral and differential forms
Know the Gibbs free energy of reaction is related to the extent of reaction
Know the condition for equilibrium in terms of chemical potential for a chemical reaction
Understand why a reaction’s equilibrium constant changes with temperature
Know the basis for finding the pressure dependence of the equilibrium constant
Terms and Definitions
Chemical potential
Heterogeneous equilibria
Gibbs free energy of reaction
van’t Hoff equation
Key Equations
First-tier
 G 
 U 
 H 
 A 
1  







 n1 T,p,n 2 ,n 3 ,
 n1 S,V,n 2 ,n 3 ,
 n1 S,p,n 2 ,n 3 ,
 n1 V,T,n 2 ,n 3 ,
p 
f  i  RT ln  f 
 pi 
G rxn  G 0rxn  RT ln Q
G 0rxn  RT ln K
 G 
G rxn  

  p,T
  ln K  H
  1   R
   
  T  p
 f p  f p  
C
D

Kp  
a
  f A p 0   f B p 0 b 


0 c
0 d
Second-tier
 K  H0  1 1 
ln  2  
  
R  T2 T1 
 K1 
K 
V0
ln  2    
dp
RT
 K1 
0
10
Phase Transitions
Concepts
Know the role of chemical potential in a phase transition
Understand how a phase transition temperature can be found from the temperature dependences
of the chemical potentials of the two phases
Know how chemical potential is related to molar entropy
Know how boiling points and freezing points change with pressure
Know the basis for the Clapeyron equation
Know what assumptions are used to modify the Clapeyron equation to become the ClausiusClapeyron equation
Understand the meaning of Clausius-Clapeyron equation in its differential and integrated forms
Be able to distinguish between 1st order phase transitions, 2nd order phase transitions and lambda
transition
Be able to give an example for each type of phase transition
Understand why kinetics can be important issue is phase transitions
Terms and Definitions
1st order phase transition
2nd order phase transition
Lambda transition
Phase
Phase transition
Clausius equation
Clausius-Clapeyron equation
Key Equations
First-tier
d
 S
dT
dp S
H


dT V TV
H vap  1 1 
p 
ln  2   
  
R  T2 T1 
 p1 
Second-tier
p 2  p1 
H  T2  T1 
V
T1
H vap
d  ln p 

R
1
d 
T
11
Mixtures and Solutions
Concepts
Know the distinction between molar quantities and partial molar quantities
Know the total volume of a mixture can be found from partial molar volumes of the components
Know why partial molar volume can be negative
Know how all partial molar quantities are defined
Know the definition of chemical potential
Understand how chemical potentials are related to each other via the Gibbs-Duhem equation
Understand how the activity of liquid component is related to the chemical potential of its vapor
Know the molecular level conditions for an ideal solution
Know how to define and ideal solution thermodynamically
Understand the thermodynamic basis for the molecular level conditions for an ideal solution
Understanding the basis for finding the Gibbs free energy and entropy of mixing
Understand the enthalpy of mixing for an ideal solution is zero
Understand the molecular level reasons why the enthalpy of mixing for an ideal solution is zero
Understand the basis for finding the freezing point depression and boiling point elevation of a
solution
Understand the basis for finding the osmotic pressure of an ideal solution
Understand how the focus of colligative properties changes from the solvent to the solute
Know the van’t Hoff factor helps distinguish strong electrolytes, weak electrolytes and
nonelectrolytes
Know how colligative properties can be used to measure the activity of solvents in a solution
Terms and Definitions
Partial molar volume
Gibbs-Duhem equation
Activity
Ebullioscopic constant
Cryoscopic constant
van’t Hoff factor
Key Equations
First-tier
 G 
1  

 n1 T,p,n 2 ,n3 ,
 V 
 V 
dV  
 dn1  
 dn 2
 n1  n 2
 n 2  n1
 A  l   *A  l 
ln a A 
RT
G mix  G  G *
aA 
pA
p*A
p A  x A p*A
1  s   1*  l   RT ln x1
n1d1  n 2d2  0
VA  VA*
H A  H*A
1  T, patm  , x1   1*  T, patm 
Second-tier
G mix  nRT x i ln x i
i
Smix  nR  x i ln x i
i
M1RTm*2
Tm 
c2  k f c2
H fus
12
Phase Diagrams
Concepts
Know the derivation of the Gibbs phase rule
Know how to apply the Gibbs phase rule to a two-component liquid-vapor phase diagram
Know how to use a tie line to find the composition of vapor and the composition of liquid in the
two phase region of a two-component liquid-vapor phase diagram for a specific temperature
and total composition
Know how to use the lever rule to determine the relative amounts of vapor and liquid in a twocomponent liquid-vapor phase diagram for a specific temperature and total composition
Understand how different volatilities between two liquids in a mixture affects the composition of
the vapor above the liquid
Understand how the two-component liquid-vapor phase diagram aid in the understanding of a
fractional distillation
Know the difference between fractional distillation and steam distillation
Know when steam distillation is a preferred separation process
Be able to identify the azeotropic composition of a mixture on a liquid-vapor phase diagram
Know why identification of azeotropes is important in the practical application of distillation as a
separation process
Know the regions in a two-component liquid-vapor phase diagram with an immiscible liquid
phase and how to apply a tie line to find compositions and the level rule to find relative
amounts
Know the regions in a two-component liquid-liquid phase diagram and how to apply a tie line to
find compositions and the level rule to find relative amounts
Know the regions in a two-component liquid-solid phase diagram and how to apply a tie line to
find compositions and the level rule to find relative amounts
Understand the advantage of knowing a solid mixture’s eutectic point
Be able to reproduce two-component liquid-solid phase diagram from a set of cooling curves
Understand the role that kinetics plays in creating solids that are not in equilibrium with their
liquid phases
Be able to identify solid-state compound formation via a congruent melting point on a twocomponent liquid-solid phase diagram
Be able to state the reaction for a specific congruent melting point
Be able to identify a peritectic point on a phase diagram
Be able to state the reaction for incongruent melting around a peritectic point
13
Terms and Definitions
Gibbs phase rule
Isopleth
Dew point curve
Bubble point curve
Tie line
Lever rule
Fractional distillation
Theoretical plate
Azeotrope
Upper consulate temperature
Lower consulate temperature
Liquidus
Solidus
Eutectic point
Eutectic composition
Eutectic temperature
Cooling curve
Congruent melting
Congruent melting point
Peritectic point
Peritectic reaction
Incongruent melting
Key Equations
First-tier
f  cp2
Second-tier


p*A
yA  x A  *
* 
 pB 1  x A   x A p A 
xA 
p
y A p*B
*
A
 y A  p*B  p*A  
14
Electrolytic Solutions
Concepts
Understand the relationships between electrical forces, electrical energies, electric potentials and
electric fields
Know conceptually what the unit of Faraday represents
Know conceptually what the dielectric constant describes
Know the distinction between conductance and conductitvity and why the distinction is
important
Know why the distinction between conductivity and molar conductivity is important for
electrolytic solutions
Know Kohlrausch’s law of independent migration for ions and its relevance in explaining the
molar conductivity of electrolytic solutions
Know how the molar conductivity of weak electrolytic solutions varies with concentration
Know how the molar conductivity of strong electrolytic solutions varies with concentration
Know how Arrhenius explained the molar conductivity of weak electrolytic solution with the
degree of dissociation parameter
Know how the Arrhenius theory of weak electrolytes fits with Ostwald’s dilution law
Know how the Arrhenius theory of weak electrolytes fits with the law of mass action
Know why the Arrhenius theory of weak electrolytes fails to explain the molar conductivites of
strong electrolytic solutions
Understand how the Debye-Huckel theory attempted to describe the charge distribution of ions
around an ion in solution via a balance between thermal energies and electrical attraction
energies
Understand the goal behind the analysis to find the charge distribution of ions in solution
Understand how the thickness of the ionic atmosphere affects the description of the interaction
between charges in solution
Understand how the nonideal behavior of an electrolytic solution is related to the Gibbs free
energy of an ideal solution
Understand that the definition of standard state of a solution affects its standard Gibbs free energy
Know the assumptions made to simplify the extended Debye-Hückel to the Debye-Hückel
limiting law
Know the range of applicability for the extended Debye-Hückel law, the Debye-Hückel limiting
law and the Davies equation
Know the standard state for ions in solution
Know the standard state for ions is used to find the measured values for other ions in solution
Know why the use of mean ionic activity coefficients is necessary
Know how to calculate the mean ionic activity coefficient for an ion in solution
15
Terms and Definitions
Faraday’s constant
Electric potential
Electric field
Dielectric constant
Conductance
Conductivity
Molar conductivity
Electrolyte
Nonelectrolyte
Degree of dissociation
Ostwald’s dilution law
Law of mass action
Debye-Hückel theory
Ionic strength
Thickness of ionic atmosphere
“Distance of closest approach”
Extended Debye-Hückel law
Debye-Hückel limiting law
Davies equation
Mean ionic activity coefficient
Key Equations
First-tier
F
1 Q1Q 2
4 0  r 2
E
G
I  GV
F
1 Q1

Q 2 40  r 2
l
A


c

W

0
1 Q1Q 2
4 0  r
I
1
N i Zi2

2 i

W
1 Q1

Q 2 4 0  r
log  j  Z2j B I
   a b  a  b
Second-tier
  
 
c  0 K
  
1 

 0 
2
(a 0  x)(b0  x)  K  c0  x  (d0  x)
 j   Zi eNi   Zi eNi e
i
i
 Z2j e 2   
ln  j 


2 0 RT  1  a 

Zi e j
kT
 kT
1
 0 2

8e I
a
RT ln  i  w    dQ
 I 
log  j   Z2j B 
  cI
 1 I 

16
Electrochemistry
Concepts
Know the difference between oxidation and reduction
Know the difference between oxidizing agent and reducing agent
Know the relationship between the conservation of charge and a balanced redox reaction
Be able to write an electrochemical reaction in line notation
Know the major application for a galvanic reaction
Be able to make a sketch that illustrates the essential features of a galvanic cell
Understand the relationship between the work done in an electrochemical reaction and its cell
potential
Know how cell potential is related to the Gibbs free energy of a reaction
Know how to use the Nernst equation to calculate the concentration dependence of the cell
potential
Be able to use the Nernst equation to calculate the cell potential in a concentration cell
Be able to use the Nernst equation to find the equilibrium constant for an electrochemical reaction
Know how to calculate the standard cell potential for an electrochemical reaction using standard
reduction potentials
Know the essential differences between a galvanic cell and an electrolytic cell
Know some applications for electrolytic reactions
Be able to make a sketch that illustrates the essential features of a galvanic cell
Know the connections between time, current and mass for an electrolytic reaction
Terms and Definitions
Oxidation
Reduction
Oxidizing agent
Reducing agent
Cathode
Anode
Redox couple
Galvanic reaction (cell)
Daniell cell
Liquid junction
Concentration cell
Nernst equation
Standard hydrogen electrode
Standard reduction potential
Electrolytic reaction (cell)
Key Equations
First-tier
we = -eE
 r G  FE
E  E0 
RT
ln Q
F
Q=It