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Thermodynamics of Interfaces

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Title: Thermodynamics of Interfaces


1
Thermodynamics of Interfaces
  • And you thought this was just for the chemists...

Courtesy of John Selker (Oregon State University)
2
Terms
Key Concept two kinds of variables Intensive do
not depend upon the amount (e.g.,
density) Extensive depend on the amount (e.g.,
mass)
  • Extensive Variables
  • S entropy
  • U internal energy
  • N number of atoms
  • V volume
  • ?? Surface area
  • Intensive Variables
  • P pressure
  • ?? Surface tension
  • T Temperature (constant)
  • ?? Chemical potential

3
Phases in the system
  • Three phases
  • liquid gaseous taut interface
  • Subscripts
  • indicates constant intensive parameter
  • g l a indicate gas, liquid, and
    interface

Gaseous phase g
Interface phase a
Liquid phase l
4
Chemical Potential
  • ??refers to the per molecule energy due to
    chemical bonds.
  • Since there is no barrier between phases, the
    chemical potential is uniform
  • ?g ?a ?l ? 2.21

5
Fundamental Differential Forms
  • We have a fundamental differential form (balance
    of energy) for each phase
  • TdSg dUg PgdVg - ?dNg (gas) 2.22
  • TdSl dUl PldVl - ?dNl (liquid) 2.23
  • TdSa dUa - ?d? (interface) 2.24
  • The total energy and entropy of system is sum of
    components
  • S Sa Sg Sl 2.25
  • U Ua Ug Ul 2.26

6
How many angels on a pin head?
  • The inter-phase surface is two-dimensional, The
    number of atoms in surface is zero in comparison
    to the atoms in the three-dimensional volumes of
    gas and liquid
  • N Nl Ng 2.27

7
FDF for flat interface system
  • If we take the system to have a flat interface
    between phases, the pressure will be the same in
    all phases (ignoring gravity), which we denote P
  • The FDF for the system is then the sum of the
    three FDFs
  • TdS dU PdV - ?dN - ?d? (system) 2.27

8
Gibbs-Duhem relationship
  • For an exact differential, the differentiation
    may be shifted from the extensive to intensive
    variables maintaining equality.
  • TdS dU PdV - ?dN - ?d? (system)
  • SadT ? d ? 2.29
  • or
  • Equation of state for the surface phase
    (analogous to Pv nRT). Relates temperature
    dependence of surface tension to the magnitude of
    the entropy of the surface.

9
Laplaces Equation from Droplet in Space
  • Now consider the effect of a curved air-water
    interface.
  • Pg and Pl are not equal
  • ?g ?l ??
  • Fundamental differential form for system
  • TdS dU PgdVg PldVl - ??(dNgdNl ) - ?d?
    2.31

10
Curved interface Thermo, cont.
  • Considering an infinitesimally small spontaneous
    transfer, dV, between the gas and liquid phases
  • chemical potential terms equal and opposite
  • the total change in energy in the system is
    unchanged (we are doing no work on the system)
  • the entropy constant
  • TdS dU PgdVg PldVl - ??(dNgdNl) - ?d?
    2.31
  • Holding the total volume of the system constant,
    2.31 becomes
  • (Pl - Pg)dV - ?d? 0 2.32

11
Droplet in space (cont.)
  • where Pd Pl - Pg
  • We can calculate the differential noting that for
    a sphere V (4?r3/3) and ? 4?r2
  • 2.34
  • which is Laplace's equation for the pressure
    across a curved interface where the two
    characteristic radii are equal (see 2.18).

12
Simple way to obtain La Places eq....
  • Pressure balance across droplet middle
  • Surface tension of the water about the center of
    the droplet must equal the pressure exerted
    across the area of the droplet by the liquid
  • The area of the droplet at its midpoint is ?r2 at
    pressure Pd, while the length of surface applying
    this pressure is 2?r at tension ?
  • Pd ?r2 2?r? 2.35
  • so Pd 2s/r, as expected

13
Vapor Pressure at Curved Interfaces
  • Curved interface also affects the vapor pressure
  • Spherical water droplet in a fixed volume
  • The chemical potential in gas and liquid equal
  • ?l ?g 2.37
  • and remain equal through any reversible process
  • d?l d?g 2.38

14
Fundamental differential forms
  • As before, we have one for each bulk phase
  • TdSg dUg PgdVg - ?gdNg (gas) 2.39
  • TdSl dUl PldVl - ?ldNl (liquid) 2.40
  • Gibbs-Duhem Relations
  • SgdT VgdPg - Ngd?g (gas) 2.41
  • SldT VldPl - Nld?l (liquid) 2.42

15
Some algebra
  • SgdT VgdPg - Ngd?g (gas) 2.41
  • SldT VldPl - Nld?l (liquid) 2.42
  • Dividing by Ng and Nl and assume T constant
  • vgdPg d?g (gas) 2.43
  • vldPl d?l (liquid) 2.44
  • v indicates the volume per mole. Use d?g d?l
    2.38 to find
  • vgdPg vldPl 2.45
  • which may be written (with some algebra)

16
Using Laplaces equation...
  • or
  • since vl is four orders of magnitude less than
    vg, so suppose (vg - vl)/vl ??vg/vl
  • Ideal gas, Pgvg RT, 2.49 becomes

17
Continuing...
  • Integrated from a flat interface (r ?) to that
    with radius r to obtain
  • where P? is the vapor pressure of water at
    temperature T. Using the specific gas constant
    for water (i.e., R/vl), and left-hand side is
    just Pd, the liquid pressure

18
Psychrometric equation
  • Allows the determination of very negative
    pressures through measurement of the vapor
    pressure of water in porous media.
  • For instance, at a matric potential of -1,500 J
    kg-1 (15 bars, the permanent wilting point of
    many plants), Pg/P? is 0.99.

19
Measurement of Pg/P?
  • A thermocouple is cooled while its temperature is
    read with a second thermocouple.
  • At the dew point vapor, the temperature decline
    sharply reduces due to the energy of condensation
    of water.
  • Knowing the dew point T, it is straightforward to
    obtain the relative humidity
  • see Rawlins and Campbell in the Methods of Soil
    Analysis, Part 1. ASA Monograph 9, 1986

20
Temperature Dependence of ?
  • Often overlooked that all the measurements we
    take regarding water/media interactions are
    strongly temperature dependent.
  • Surface tension decreases at approximately one
    percent per 4oC!
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