Contents

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Contents
1. Introduction
9. Liquid Handling
2. Fluids
10.Microarrays
3. Physics of Microfluidic
Systems
11.Microreactors
12.Analytical Chips
4. Microfabrication Technologies
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13.Particle-Laden Fluids
5. Flow Control
a. Measurement Techniques
6. Micropumps
7. Sensors
b. Fundamentals of
Biotechnology
8. Ink-Jet Technology
c. High-Throughput Screening
Microfluidics - Jens Ducrée
Fluids: Thermodynamics
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2. Fluids
1. General Characteristics
2. Dispersions
3. Thermodynamics
4. Transport Phenomena
5. Solutions
6. Surface Tension
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7. Electrical Properties
8. Optical Properties
9. Biological Fluids
Microfluidics - Jens Ducrée
Fluids: Thermodynamics
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2.3. Thermodynamics
1. Heat and Temperature
2. Heat Capacity
3. Chemical Potentials
4. Kinetic Theory of Gases
5. Compressibility
6. Thermal Expansion
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7. Real Gases
8. Vapor Pressure
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Fluids: Thermodynamics
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2.3.1. Heat and Temperature
 Thermal energy per molecule




In thermal equilibrium
Number of degrees of freedom f
Boltzmann constant
Heating 1 mole of ideal gas by 1 K consumes 4.16 J per DoF
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 Three translational DoFs
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Fluids: Thermodynamics
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2.3.1. Heat and Temperature
 Mean kinetic energy
 Combination yields for mean (random, thermal) velocity
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2.3. Thermodynamics
1. Heat and Temperature
2. Heat Capacity
3. Chemical Potentials
4. Kinetic Theory of Gases
5. Compressibility
6. Thermal Expansion
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7. Real Gases
8. Vapor Pressure
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Fluids: Thermodynamics
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2.3.2. Heat Capacity
 Raising temperature of N particles by T takes energy
 Heat capacity
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 Specific heat capacity
 Molar heat capacity
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Fluids: Thermodynamics
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2.3. Thermodynamics
1. Heat and Temperature
2. Heat Capacity
3. Chemical Potentials
4. Kinetic Theory of Gases
5. Compressibility
6. Thermal Expansion
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7. Real Gases
8. Vapor Pressure
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Fluids: Thermodynamics
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2.3.3. Internal Energy
 Internal energy U
 State property
 Conservation of energy
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 Amount of transferred heat Q
- Q > 0: heat absorbed by system
 (Expansion) work W = p V
- W > 0: system delivers work, i.e. system spends energy
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Fluids: Thermodynamics
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2.3.3. Enthalpy
 Enthalpy (state property)
 Chemical reactions normally at constant p
 Heat energy absorbed or released to system at constant p
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 Transferred heat Qp= change in enthalpy
 No volumetric expansion
- Transferred heat = change in internal energy
 Example:
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Fluids: Thermodynamics
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2.3.3. Entropy
 Entropy
 Probability Wprob of finding system in given state
 Entropy of „universe“
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 Entropy of environment Senv
 Entropy of system under investigation S
 Stot constantly grows
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2.3.3. Gibbs Free Enthalpy
 Processes at constant T and p
 Typical for chemical reactions
 Can process occur spontaneously?
 Gibbs free enthalpy G = H - TS
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 G < 0 for spontaneous process
 Decrease in enthalpy H
 Increase in entropy S
 High temperature T
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Fluids: Thermodynamics
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2.3. Thermodynamics
1. Heat and Temperature
2. Heat Capacity
3. Chemical Potentials
4. Kinetic Theory of Gases
5. Compressibility
6. Thermal Expansion
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7. Real Gases
8. Vapor Pressure
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2.3.4. Kinetic Theory of Gases
 Gas Pressure
 Force perpendicular to surface A
 Scalar
 Isotropic
 Units




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1 Pa = 1 N m-2
1 Torr (= mm Hg) = 133.4 Pa
1 mbar = 1 hPa
1 psi = 6897 Pa
 Standard pressure
 1 atm = 1013 hPa = 1013 mbar =
=760 Torr = 14.7 psi
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2.3.4. Kinetic Theory of Gases
 Molecular picture
 Particle density: N / V
 Only particles in defined sub-volume (A x v x t ) have chance to hit
wall within given time t
 1/3 of velocity vectors statistically perpendicular to surface A
 1/2 of them pointing towards wall
 Number of collisions (N / V ) x ( A x v x t ) / 6
 Each particle transfers twice its momentum: 2 x mv = F t
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v t
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2.3.4. Kinetic Theory of Gases
 Bernoulli equation
 By replacing v² with v² (mean square velocity)
 Substitute v² by thermal velocity
 Equation of state for ideal gas
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particles
moles
 # molecules N
 # moles n
 Gas constant Rg = 8.31 J K-1 mol-1
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2.3.4. Kinetic Theory of Gases
 (Trivial) conclusions from equation of state
 Law of Boyle-Mariotte
 Law of Gay-Lussac
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 Law of Charles
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2.3.4. CV and Cp for Gases
 Heat capacity of gases
 At constant volume
-
CV = ½ f N kB
 At constant pressure
- Volumetric expansion associated with mechanical work
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heat
mech. work
 Equivalence of thermal and mechanical energy
 1 cal = 4.18 J
 1842: Robert Mayer and J. P. Joule
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2.3.4. Adiabatic Change of Condition
 Adiabatic process
 No exchange of thermal energy Q = 0
 E.g., under thermal insulation  U = – W
 Complete conversion (internal) heat  pneumatic work
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 Insertion of equation of state and CV
CV = ½ f N kB
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Fluids: Thermodynamics
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2.3.4. Adiabatic Change of Condition
 Relationship for adiabatic process
„non-adiabatic“ gas laws
 Adiabatic coefficient
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 Poisson equations
 Compare to „non-adiabatic“ gas laws
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2.3.4. Mean Free Path
 Collisional cross section for given gas
 Mean free path scales with
 Inverse of particle density
 Inverse of collisional cross-section of particles
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thermal motion of targets
 Example: H2 at p = 1013 hPa
 lmfp = 270 nm
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2.3. Thermodynamics
2.3.1. Heat and Temperature
2.3.2. Heat Capacity
2.3.3. Chemical Potentials
2.3.4. Kinetic Theory of Gases
2.3.5. Compressibility
2.3.6. Thermal Expansion
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2.3.7. Real Gases
2.3.8. Vapor Pressure
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2.3.5. Compressibility
 Compressibility of fluids
 Isothermal compressibility for ideal gas
 Bulk modulus
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p V = const.
 Differentiation of modified (adiabatic) law of Boyle-Mariotte
 Adiabatic compressibility
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Fluids: Thermodynamics
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2.3.5. Compressibility
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2.3. Thermodynamics
2.3.1. Heat and Temperature
2.3.2. Heat Capacity
2.3.3. Chemical Potentials
2.3.4. Kinetic Theory of Gases
2.3.5. Compressibility
2.3.6. Thermal Expansion
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2.3.7. Real Gases
2.3.8. Vapor Pressure
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2.3.6. Thermal Expansion
 Thermal expansion coefficient
 Derivation from equation of state for (ideal) gases
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 Expansion of cube
 Linear approximation
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2.3.6. Thermal Expansion
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2.3. Thermodynamics
2.3.1. Heat and Temperature
2.3.2. Heat Capacity
2.3.3. Chemical Potentials
2.3.4. Kinetic Theory of Gases
2.3.5. Compressibility
2.3.6. Thermal Expansion
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2.3.7. Real Gases
2.3.8. Vapor Pressure
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2.3.7. Real Gases
 Van-der-Waals equation
 Volume per mole Vn
 „Internal pressure“ a/Vn²
- Attractive forces between molecules
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 Parameter for strength of interaction a
 Covolume b
- Spatial extension of molecules subtracted from overall volume
- At low pressures negligible due to large volume per mole Vn
 Joule-Thomson effect
 Change in temperature during rapid expansion
 Work against intermolecular forces
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2.3. Thermodynamics
2.3.1. Heat and Temperature
2.3.2. Heat Capacity
2.3.3. Chemical Potentials
2.3.4. Kinetic Theory of Gases
2.3.5. Compressibility
2.3.6. Thermal Expansion
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2.3.7. Real Gases
2.3.8. Vapor Pressure
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2.3.8. Vapor Pressure
 Coexistence of liquid and gaseous state




Closed vessel
Vapor forms above liquid
Saturated vapor pressure
Boiling
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Standard
Pressure
 Temperature dependence
Boiling
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2.3.8. Vapor Pressure
 Vapor pressure curve
 Coexistence of liquid and vapor
 Restricted to 1-dimensional curve
- Above only vapor
- Below only liquid
 Critical point
 Phases „converge“
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2.3.8. Vapor Pressure
 Absolute humidity abs
 Concentration of mass, measured in g / m3
 Relation to partial pressure of water pwater
- Mass of water molecule mwater
 Relative humidity
 rel referred to abs at saturation
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 Heat of vaporization 
 E per mass to „escape“ liquid phase
 Equation of Clausius and Clapeyron
 Temperature T
 Derivative of vapor pressure curve dp / dT
 Difference between specific volumes Vm
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