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Chrom-Ed Book Series
Raymond P. W. Scott
Dispersion in
ChromatographyColumns
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COPYRIGHT @2003 by LIBRARY4SCIENCE, LLCALL RIGHTS RESERVED
Neither this book or any part may be reduced or transmitted in anyform or by any means, electronic or mechanical , includingphotocopying, microfilming, and recording or by any informationstorage and retrieved system without permission in writing from thepublisher except as permitted by the in-user license agreement.
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Contents
Introduction to the Rate Theory..............................................................1The Summation of Variances..................................................................2
The Alternative Axes of a Chromatogram..........................................9The Random Walk Model.................................................................13Dispersion Processes that take Place in an LC Column...................22
The Multipath Process...................................................................23
Longitudinal Diffusion..................................................................24The Diffusion Process...................................................................24The Resistance to Mass Transfer in The Mobile Phase................29The Resistance to Mass Transfer in the stationary Phase.............30Resistance to Mass Transfer Dispersion.......................................31Diffusion Controlled Dispersion in the Stationary Phase............34
Diffusion Controlled Dispersion in the Mobile Phase.................35Effect of Mobile Phase Compressibility On the HETP Equation for aPacked GC Column...........................................................................37The Van Deemter Equation...............................................................43
Alternative Equations for Peak Dispersion ..........................................55The Giddings Equation.....................................................................56The Huber Equation..........................................................................57The Knox Equation...........................................................................59The Horvath and Lin Equation..........................................................61The Golay Equation..........................................................................61
Experimental Validation of the Van Deemter Equation...................66The Effect of the Function of (k') on Peak Dispersion.....................82
Summary................................................................................................84
References ............................................................................................86
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Introduction to the Rate Theory
The separation of a solute pair in a chromatographic system depends on
moving the peaks apart in the column and constricting their dispersion
so that the two solutes are eluted discretely. The factors that control
retention have been discussed in Book 7 and in this book the processes
of peak dispersion will be considered together with the means by which
peak dispersion can be minimized.
Solute equilibrium between the mobile and stationary phases is never
achieved in the chromatographic column except possibly at the
maximum of a peak. To circumvent this non equilibrium condition and
allow a simple mathematical treatment of the chromatographic process,
Martin and Synge (1) borrowed the plate concept from distillation
theory and considered the column consisted of a series of theoretical
plates in which equilibrium could be assumed to occur. In fact each
plate represented a 'dwell time' for the solute to achieve equilibrium atthat point in the column and the process of distribution could be
considered as incremental. This approach has been discussed in Book
6.
Employing this concept an equation for the elution curve can be easily
obtained and, from that basic equation, others can be developed that
describe the various properties of a chromatogram. Such equations
have permitted the calculation of efficiency, the number of theoretical
plates required to achieve a specific separation and among manyapplications, elucidate the function of the heat of absorption detector.
The Plate Theory, however, does little to explain how the efficiency of
a column may be changed or, what causes peak dispersion in a column
in the first place. It does not tell us how dispersion is related to column
geometry, properties of the packing, mobile phase flow-rate, or the
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physical properties of the distribution system. Nevertheless, it was not
so much the limitations of the Plate Theory that provoked Van Deemter
et al (2) (who were chemical engineers and mathematicians) to
develop, what is now termed the Rate Theory for chromatographic
dispersion, but more to explore an alternative mathematical approach toexplain the chromatographic process. Virtually all basic
chromatography theory evolved over the twenty five years between
1940 and 1965 and it was in the middle of this period that Van Deemter
and his colleagues presented their Rate Theory concept in (1956).
Since that time, other Rate Theories have been presented, together with
accompanying dispersion equations and in due course each will be
discussed, but most were very similar in form to that of Van Deemter
et al. It is interesting to note, however, that, even after thirty five years
of chromatography development, the equation that best describes band
dispersion in practice is still the Van Deemter equation. This is
particularly true for columns operated around the mobile phase
optimum velocity where the maximum column efficiency is obtained.
The purpose of the Rate Theory is to help understand the processes that
cause dispersion in a chromatographic column and to identify those
properties of the chromatographic system that control it. Such
information will allow the best column to be designed to effect a given
separation in the most efficient way. However, before discussing the
Rate Theory some basic concepts must be introduced and illustrated.
The Summation of Variances
The width of the band of an eluted solute relative to its proximity to its
nearest neighbor determines whether two solutes are resolved or not.
The ultimate band width as sensed by the detector is the result of a
number of individual dispersion processes taking place in the
chromatographic system, some of which take place in the column itself
and some in the sample valve, connecting tubes and detector (see book
10). In order to determine the ultimate dispersion of the solute band it
is necessary to be able to calculate the final peak variance. This is
achieved by taking into account all the individual dispersion processes
that take place in a chromatographic system. It is not possible to sum
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the band widths (standard deviation or ()) resulting from eachindividual dispersion process to obtain the final band width, but it is
possible to sum all the respective variances. However, the summation
of all the variances resulting from each process is only possible if each
process is non-interacting and random in nature. That is to say, theextent to which one dispersion process progresses is independent of the
development and progress of any other dispersion process.
Thus, assuming there are (n) non-interacting, random dispersive
processes occurring in the chromatographic system, then any process
(p) acting alone will produce a Gaussian curve having a variance p
2
,
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Hence,
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where, (
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) is the variance of the solute band as sensed by the detector.
The above equation is the algebraic enunciation of the principle of the
summation of variances and is fundamentally important. If the
individual dispersion processes that are taking place in a column can be
identified, and an expression for the variance arising from each
dispersion process evaluated, then the variance of the final band can be
calculated from the sum of all the individual variances. This is how the
Rate Theory provides an equation for the final variance of the peak
leaving the column.
The Alternative Axes of a Chromatogram
An elution curve of a chromatogram can be expressed using parameters
other than the volume flow of mobile phase as the independent variable.The Plate theory provides an equation that expresses the retention and
standard deviation of a peak in terms volume flow of mobile phase.
However, instead of using milliliters of mobile phase, as the
independent variable, solute concentration in the mobile phase can be
related, time, or distance traveled by the solute band along the column
and proportionally the same chromatogram will be obtained. This is
illustrated in figure (1)
As the curves are describing the same chromatogram, by proportion,
the ratio of the variance to the square of the retention, in the respective
units in which the independent variables are defined, will all be equal.
Consequently, v
2
V r2
= x
2
l 2=
t2
t r2
where v, x and t are the standard deviations of the elution curveswhen related to the volume flow of mobile
phase, the distance traveled by the solute along
the column and time, respectively.and Vr, l and tr refer to the retention volume, column length
and retention time, respectively.
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2 v
v
2 x
x
2 t
tF l o w o f M o b i l e P h a s e
i n P l a t e V o l u m e s
R e t e n t i o n T i m e D i s t a n c e T r a v e l l e d
a l o n g C o l u m n
Figure 1 Alternative Axes of a Chromatogram
Now, from the Plate Theory (see book 6) it has been shown that,
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Thus,
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and
Therefore,l
n=
x2
l
The ratio, (l
n), (the column length divided by the number of theoretical
plates in the column) has, for obvious reasons, become termed the
Height Equivalent to the Theoretical Plate (HETP) and has been given
the symbol (H). However, it is seen that (H) is numerically equal to, ,
which is, in fact, the variance per unit length of the column. Thus, the
function, , is the variance that the Rate Theory will provide an explicit
equation to define and can be experimentally calculated for any column
from its length and column efficiency. It follows that the equations that
give a value for, (H), the variance per unit length of the column, have
been termed HETP equations.
To develop an HETP equation it is necessary to first identify the
dispersion processes that occur in a column and then determine the
variance that will result from each process per unit length of column.
The sum of all these variances will be (H), the Height of the
Theoretical Plate, or the total variance per unit column length. There
are a number of methods used to arrive at an expression for thevariance resulting from each dispersion process and these can be
obtained from the various references provided. However, as an
example, the Random-Walk Model introduced by Giddings (3) will be
employed here to illustrate the procedure. The theory of the Random-
Walk processes itself can be found in any appropriate textbook on
probability (4) and will not be given here but the consequential
equation will be used.
The Random Walk Model
The random-walk model consists of a series of step-like movements for
each molecule which may be positive or negative the direction being
completely random. After (p) steps, each step having a length (s) the
average of the molecules will have moved some distance from the
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starting position and will form a Gaussian type distribution curve with
a variance of s2 .
Now according to the random-walk model,
= s p (1)
Equation (1) can be used in a general way to determine the variance
resulting from the different dispersion processes that occur in an
chromatography column. The application of equation (1) is simple, the
problem that often arises is the identification of the average step and
sometimes the total number of steps associated with the particular
process being considered. As an illustration of its use it will be used to
the problem of obtain an expression for the radial dispersion of a
sample when it is placed on a packed column in the manner of Horne et
al. (5).
When a stream of mobile phase carrying a solute impinges upon a
particle, the stream divides and flows around the particle. Part of the
divided stream then joins other split streams from neighboring
particles, impinges on another and divides again. When a sample is
placed on the column at the center of the packing, initially it is in acondition of non-radial equilibrium, but as a result of this process the
sample spreads across the column during passage through the column
and eventually achieves radial equilibrium (the concentration of solute
is constant across a cross section of the column. Early work in liquid
chromatography, used relatively low inlet pressures and, thus, samples
could be injected directly onto the column with a syringe through an
appropriate septum device as in gas chromatography. This method of
injection often resulted in radial equilibrium never being achieved by
the solutes before they were eluted. The introduction of the sample
valve, however, aids in establishing radial equilibrium early in the
separation but unless some special spreading device is employed at the
front of the column, it will not necessarily occur at the point of
injection. The stream splitting process is depicted in figure (2). If a
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particular molecule is considered passing round a particle, it will suffer
a lateral movement that can be seen to be given by,
Lateral Movement/Particle =dp
2cos
d p
e
Figure 2. The Mechanism of Radial Dispersion
It follows, that the average lateral step will be,dp
2
cos
2
+
2
d = dpEmploying the random walk function, the radial variance will be given
by:- 2 = Num ber of Steps ) X Step Length ) 2 (2)
Now assuming one lateral step is taken by a molecule for everydistance (jdp) that it moves axially, then, (n) the number of steps is
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given by:-
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where (l) is the distance traveled axially by the solute band.
Thus, substituting for (n) in equation (2),
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In practice the value of (j) will lie between 0.5 and 1.0, but, for
simplicity the value of (j) will be taken as unity. This implies that one
lateral step will be taken by a given molecule for every step traveled
axially equivalent to one particle diameter .
Thus,
or, (3)
Consider a sample injected precisely at the center of a 4 mm diameter
LC column. Employing equation (3) allows the distance traveled
axially by the solute band before the radial standard deviation of the
sample of solute is numerically equal to the column radius to be
calculated. That is, the band has now spread evenly across the column
and the solute is in radial equilibrium.
For the conditions given above R = 0.2.
Thus, substituting this value in equation (3),
or, l =0 . 2
( )2
d p(4)
The distance that a solute band must pass along a column before a
sample, injected at the center of the packing, is evenly spread across its
diameter, can be calculated for columns packed with different sized
particles using equation (4). The results are shown as a graph relating
length against particle diameter in figure (3). The particle diameter
range normally employed in liquid chromatography is about 2-25
micron and so from figure 3, it is clear that radial equilibrium wouldnever be achieved for those column lengths commonly in use in LC.
Despite the lack of radial equilibrium, however, if the column packing
is completely homogeneous throughout the column length, then the
column efficiency should not be impaired. Unfortunately, ideal packing
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conditions are not always achieved and channeling often occurs, under
which circumstances lack of radial equilibrium could result in the
column efficiency being reduced with consequent loss in resolution. To
ensure radial equilibrium, it must either be achieved on injection (using
sample distribution device) or by employing narrow bore columnswhere radial equilibrium is more quickly reached. The latter
alternative, however, will depend on the resolution required and the
nature of the sample.
0
5 0 0
1 0 0 0
1 5 0 0
2 0 0 0
2 5 0 0
C
o
lu
m
n
L
en
g
th
T
ra
v
ersed
b
y
S
o
lu
te
(cm
)
0 1 0 2 0 3 0
P a r t i c l e D i a m e t e r ( m )
Figure 3. Graph of Column Length Traveled by the Solute Before
Radial Equilibrium is Achieved against Particle Diameter
Dispersion Processes that take Place in an LC Column
There are four basic dispersion processes that can occur in a packed
column that will account for the final band variance. They are,
Multipath dispersion, dispersion from Longitudinal Diffusion,This eBook is protected by Copyright law and International Treaties. All rights are reserved. This book is covered by an End User Licensee
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dispersion from the Resistance to Mass Transfer in the Mobile Phase
and dispersion from the Resistance to Mass Transfer in the Stationary
Phase. All these processes are random and essentially non-interacting
and, therefore, provide individual contributions of variance that can be
summed to produce the final band variance.
The Multipath Process
In a packed column the solute molecules will describe a tortuous path
through the interstices between the particles and obviously some will
travel shorter paths than the average and some longer paths.
Consequently, some molecules will move ahead of the average and
some will lag behind thus causing band dispersion. The multipath
effect is illustrated in figure (4).
d L
Figure 4. Dispersion by the Multipath Effect
The Multipath effect can be applied to the Random Walk Model. The
average path length is equivalent to the mean diameter of the particle(dp) and thus the number of steps will be equivalent to the column
length divided by the average step i.e. .
Thus, applying equation (1),
or,
Dividing by the column length, (l), the variance per unit length or of
the multipath dispersion will be obtained and, thus, the multipath
contribution (HM) to the overall height of the theoretical plate (H),
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In fact, Van Deemter introduced a constant (2) to account for theinhomogeneity of packing so his expression for the Multipath
contribution became,
HM = 2 d p
For an ideally packed column (l) will be 0.5, and under which
circumstances the value fro (HM) reverts to,
.Longitudinal Diffusion
If a local concentration of solute is placed at the midpoint of a tube
filled with either a liquid or a gas the solute will slowly diffuse to
either end of the tube. It will first produce a Gaussian distribution with
a maximum concentration at the center and, finally, when the solutereaches the end of the tube, 'end' effects occur and the solute will
continue to diffuse until there is a constant concentration throughout
the length of the tube. The process is illustrated in Figure 5.
M o b i l e P h a s e
S a m p l e
Figure 5. Longitudinal Diffusion
Before dispersion due to longitudinal dispersion is discussed some
basic principles of diffusion need to be considered.
The Diffusion Process
Diffusion processes play important parts in peak dispersion. The
process not only contributes to dispersion directly (i.e., longitudinal
diffusion), but also helps to reduce the dispersion that results from
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solute transfer between the two phases. Consider the situation depicted
in figure 6.
d x
D d c
d xm x =
A
B
D d c
d xm
x + d x = +D d c
d x( )d
d xd x
d c
d t
1 c m
1 c m
S a m p l e I n j e c t e d
x
D i f f u s i o n
C
Figure 6. The Diffusion Process
Consider a sample of solute is introduced in plane (A), (plane (A)
having unit cross-sectional area). Solute will diffuse according to
Fick's law in both directions ( x) and, at a point (x) from the sample
point, according, the mass of solute transported across unit area in unittime (mx) according to Fick will be given by,
(5)
where (Dm) is the Diffusivity of the solute in the fluid.
and is the concentration gradient at (x).
Now, mass of solute leaving the slice (dx) thick, at (x+dx), i.e.,
(mx+dx), is,
Thus, the net change in mass per unit time in the slice (dx) thick will be
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or
Now as ,
then
or,d c
d t= D m
d 2 c
d x 2(6)
Now, this is a standard differential equation and one solution to this
equation, which can be proved by appropriate differentiation, takes the
Gaussian form as follows:
Now, from the Plate Theory (see book 6),
,
where (n) is the variance of the Gaussian curve.
Now, (n) is the volume variance of the Gaussian curve ( i.e., ), then, bycomparison, (2Dmt) will be the length variance of the concentration
curve where (t) is the elapsed time. Consequently, if a differential
equation of the form is derived that describes some form of dispersion
that arises from a random diffusion process, then the solution will be a
Gaussian function and, more important from the point of view of theRate Theory, the Gaussian curve will have a variance given by (2Dmt).
Thus, if , the solution of the equation is a Gaussian function, and, for
that equation, 2 = 2 D m t (7)
Ordinary diffusion is the result of random molecular movement in first
one direction and then another and thus, resembles the Random Walk
Model. Uhlenbeck and Ornstein (8), derived the following expression
for the overall standard deviation () arising from diffusion process,
= 2 D m t( )0 . 5
where (t) is the time period over which the process occurs,
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and Dm is the Diffusivity of the solute in the mobile phase.
Actually, (t) is the time the solute spends in the moving phase and thus,
is given by, t =l
u, where (l) and (u) is the length of the column and the
linear mobile phase velocity respectively.
Thus,
and
Therefore, dividing by l to obtain the variance per unit length,
2
l= H L =
2 D mu
In the same manner as the constant () introduced by Van Deemter intothe function for multipath dispersion, Van Deemter also introduced a
constant () into the Longitudinal Dispersion contribution to varianceto account for some packing inhomogeneity. As a consequence, the
expression for the Diffusion contribution to the variance per unit length
of the column became,
HL
=2 D m
u(8)
To be precise, there should be a second longitudinal diffusion
contribution to the overall variance that would arise from the
stationary phase. The same method of derivation can be used but the
time the solute spends in the stationary phase is now, is now a function
of the capacity ratio of the column, (k').
Thus,
where (t"o) is the kinetic dead time, (see book 6)(k") is the kinetic capacity ratio.
The kinetic dead time and the kinetic capacity factors are calculated
from the kinetic dead volume as opposed to the thermodynamic dead
volume
Then from (7),
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where (Ds) is now the solute Diffusivity in the stationary phase.
However, in this case, over the time period (tr), a fraction of time is
spent by the solute in the stationary phase and, thus,
Now, again noting that ,
Noting, again that, (HD(s)), the contribution to the variance per unit
length, will be . Then, the contribution to the total variance per unit
length for the column from longitudinal diffusion in the stationary
phase will be
i.e., . (9)
Introducing a packing factor the magnitude of which will depend on
the quality of the packing, the contribution to the variance per unit
length from diffusion in the stationary phase (HL(S))is given by,
HL ( S )
=2 2 k ' D S
uwhere, DSis the Diffusivity of the solute in the stationary phase
The total contribution to (H) from longitudinal diffusion will thus be:-
or, H L =2 1 D m
u1 + k '( ) (10)
where,
It is seen from equation (10) that the longitudinal diffusion term is a
function of (k') the capacity factor of the solute. While this could be
significant in an LC capillary column systems, where the film of
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stationary phase could be continuous along the length of the column, it
will not be so in a packed column. The stationary phase in a packed
column is broken into segments between each particles and between
each pore in each particle so free continuous diffusion in the stationary
phase would be impossible. It follows that the longitudinal diffusionterm for packed columns should be independent of the k' of the solute
or, very nearly so, and in practice the effect of longitudinal diffusion in
the stationary phase is ignored.
The Resistance to Mass Transfer in The Mobile Phase
As a solute band progresses along a column, the solute molecules are
continually transferring from the mobile phase into the stationary phase
and back from the stationary phase into the mobile phase. This transfer
process is not instantaneous, because a finite time is required for the
molecules to traverse (by diffusion) through the mobile phase in order
to reach, and enter the stationary phase. Thus, those molecules close to
the stationary phase will enter it almost immediately, whereas those
molecules some distance away from the stationary phase will find their
way to it a significant interval of time later. However, as the mobile
phase is moving, during this time interval while they are diffusing
towards the stationary phase boundary, they will be swept along the
column and thus dispersed away from those molecules that were closeand entered it rapidly. The dispersion resulting from the resistance to
mass transfer in the mobile phase is depicted in figure 7.
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1 2
1 2 3 4
5 6
1 2 3 4 5 6
1 2 35
3 45 6
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
46
Figure 7. Resistance to Mas Transfer in the Mobile Phase
The diagram shows 6 solute molecules in the mobile phase and those
closest to the surface (1 and 2) enter the stationary phase immediately.
During the period, while molecules 3 and 4 diffuse through the mobile
phase to the interface, the mobile phase moves on. Thus, when
molecules 3 and 4 reach the interface they will enter the stationary
phase some distance ahead of the first two. Finally, while molecules 5
and 6 diffuse to the interface the mobile phase moves even further
down the column until molecules 5 and 6 enter the stationary phase
further ahead of molecules 3 and 4. Thus, the 6 molecules, originally
relatively close together, are now spread out in the stationary phase.
This explanation is a little over-simplified, but gives a correct
description of the mechanism of mass transfer dispersion.
The Resistance to Mass Transfer in the stationary Phase
The resistance to mass transfer in the Stationary phase is depicted infigure 8.
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2 1
4 3 2 1
5 6
1 2 3 45 6
3 4 5 6
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
S t a t i o n a r y P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
M o b i l e P h a s e
6 5 4 3 2 1
Figure 8. Resistance to Mass Transfer in the Stationary Phase
The dispersion resulting from the resistance to mass transfer in the
stationary phase can be described in the same way as that in the mobile
phase. Molecules close to the surface of the stationary phase, will leave
and enter the mobile phase before those that have diffused farther into
the stationary phase and, thus, have further to diffuse back to the
surface. Consequently, during the period required for the solute
molecules to diffuse to the stationary phase surface, those moleculesthat were close to the surface will be swept along by the moving phase
and dispersed from those molecules still diffusing to the surface. In
figure 6,molecules 1 and 2, (the two closest to the surface) will enter
the mobile phase and begin moving with the mobile phase along the
column. This process will continue while molecules 3 and 4 diffuse to
the interface at which time they, also, will enter the mobile phase and
start following molecules 1 and 2 down the column. All four molecules
will continue their journey down the column while molecules 5 and 6
diffuse to the mobile phase/stationary phase interface. By the time
molecules 5 and 6 enter the mobile phase, the other four molecules will
have been smeared along the column and the original 6 molecules will
have suffered dispersion.
Resistance to Mass Transfer Dispersion
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Both the resistance to mass transfer in the mobile phase and that in the
stationary phase, can be treated quantitatively using the random walk
model. Recalling that if each molecule of a group takes a series of
steplike movements, (positive or negative) the direction being
completely random, then after (p) steps have been taken, each stephaving an average length (s), the average of the molecules will have
moved some distance from the starting position and will form a
Gaussian type distribution curve with a variance of2,where
or
In the first instance, consider that the distribution is energy controlled
and not diffusion controlled, thus, a solute molecule will desorb from
the stationary phase when it randomly has sufficient kinetic energy tobreak its association with a molecule of stationary phase (see book 1).
Similarly, a molecule will be absorbed under the same conditions.If (kd) is the desorption rateconstant then the mean desorption time
(td) for the adsorbed molecule will be . Correspondingly, if the
adsorption rate constant is (ka), then the mean adsorption time for a
free molecule in the mobile phase will be .
Consider a peak moving down a column. During this migration
process, adsorption and desorption steps will constantly and frequently
occur and each occurrence will be a random event. Now a desorption
step will be a random movement forward as it releases a molecule into
the mobile phase. Conversely, an adsorption step will be a random
movement backward, as it is a period of immobility for the molecule
while it resides in the stationary phase and the rest of the zone moves
forward. The total number of random steps, taken as the solute mean
position moves a distance along the column, is the number of forward
steps plus the number of backward steps. Now the distribution of the
solute is dynamic and is also an equilibrium system, consequently, eachdesorption step must be followed by an adsorption step. It follows that
the total number of steps will be twice the number of adsorption steps
that take place in the migration period.
On average, a molecule will remain in the mobile phase a time (ta)
before it is adsorbed. During this time, it will be moving at the meanThis eBook is protected by Copyright law and International Treaties. All rights are reserved. This book is covered by an End User Licensee
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velocity of the mobile phase (u) and will, thus, move a distance (uta).
Thus, in moving a distance , the total number of adsorptions will be
and the total number of steps including the adsorption and desorption
steps will be . It also follows, from the Random Walk Model that,
where
It is now necessary to determine the average step length (s) to obtain an
expression for (H).
The step length is that length moved by the molecule relative to that ofthe zone center and, while the molecule has move (vta) during time
(ta), the zone center has also moved. Now, it was shown in the Plate
theory that the zone velocity is where (k") is the dynamic capacity
ratio of the solute.
Consequently, .
and, ,
i.e.,
In practice, it is more convenient to express (H) in terms of (t d) as
opposed to (ta). The ratio of the mean phase residence times is the time
the solute spends in the mobile phase divided by the time spent in the
stationary phase,
Thus,
and H R M T =2 ( k " ) 2
1 + k "( )2
ut dk "
=2 k "
1 + k "( )2
u t d (11)
Equation (11), is derived from the approximate random walk theory,
however, it is rigorously correct and applies to heterogeneous surfaces
containing wide variations in properties as well as to perfectly uniform
surfaces. It can also be used as the starting point for the random walk
treatment of diffusion controlled mass transfer similar to that which
takes place in the stationary phase in GC and LC columns.
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Diffusion Controlled Dispersion in the Stationary Phase
The difference between diffusion controlled dispersion and dispersion
resulting from adsorption and desorption processes is that the transfer
process is concentration controlled. Reiterating equation (7),
.
Thus, during solute transfer between the phases, (t) is now the average
diffusion time (tD) and () is the mean distance through which thesolute diffuses, i.e., the depth or thickness of the film of stationaryphase (df).
Thus, or (12)
where (DS) is the Diffusivity of the solute in the stationary phase.
Substituting (tD) for (td) from (12) in (11),
H M T S =q k "
1 + k "( ) 2d f
2
D Su (13)
where (q) is a configuration factor.
The constant (q) accounts for the precise shape of the 'pool' of
stationary phase which, for a uniformly coated GC capillary column, (q
= 2/3). Diffusion in 'rod' shaped and 'sphere' shaped bodies, (e.g.,
paperchromatography and LC) (q=1/2 and 2/15), respectively (7).
For a GC capillary column,
(14)
and a close approximation for an LC or GC packed column, (HMTS)
would be given by
H M T S =2 k "
1 5 1 + k "( ) 2d f
2
D Su . (15)
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Diffusion Controlled Dispersion in the Mobile Phase
Dispersion processes in the mobile phase will also be diffusion
controlled, thus, again reiterating equation (7),
While in the mobile phase a solute molecule must traverse from
localities of high velocity (near the center of a capillary column or the
center of an inter-particle channel) to that of low velocity (the interface
between the two phases at the capillary column walls or, in the packed
column, the surface of the particles). Let the "exchange time' between
the two extreme velocities be (tm). Now, the distance between the
extremes of velocity will depend on the geometry of the column
system, but in general it can be assumed a molecule must diffuse adistance (mdm) to move from one velocity extreme to the other.Depending on the column (tubular or packed), and on the homogeneity
of the packing, (particle size and shape) the value of (m) may rangewidely from much less than unity to significantly greater than unity.
Now, from equation (7),
(=mdp) and (t=tm)
Thus,
or t m = m
2
2 D md p
2. (16)
Now, in the equation from the Random walk concept,
or
In addition, = tmu andor . (17)
Substituting for (tm) from (16) in (17)
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Now,
Thus, H M T M = 2
l=
m2
2 D md p
2 u (18)
Equation (21) applies to all types of columns each requiring a different
constant (m) which is partly determined by the geometry of thedistribution system and partly by the capacity ratio of the solute. A
function for (m) has not been developed for packed LC or GCcolumns, but due to the geometric simplicity Golay (8) was able to
develop the function for the capillary column ,viz.
and thus, for a capillary column,
H M T M =1 + 6 k " + 1 1 k " 2
2 4 1 + k " 2
2r 2
2 D mu . (19)
The argument used to develop the function describing (tm) for a
capillary column is similar to that for the packed column but (r), the
column radius, replaces (dp) the particle diameter.
Due to the varying physical nature of the different packings, it appears
column, but it was suggested by Klinkenberg and Purnell that as no one
has developed a specific function for () for a packed columns,
that the function,
(developed by Golay for the capillary column) could also be used for
packed GC and LC columns. However, in a packed column. the flow
patterns in interstices between the particles is very complex and the
eddies and pseudo turbulence that are generated between the particles
greatly increases the effective diffusivity of the solute in the mobile
phase. In fact, the magnitude of equation (18) can be so reduced by thelarge increase in (Dm) that the overall contribution to the peak
dispersion can become small enough to be ignored.
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Summarizing,, the rate theory provides the following equations that
describe the variance per unit length (H) for four different columns.
1. The Open Tubular GC Column,
(20)
2. The Packed GC Column
(21)
This equation is basically that derived by Van Deemter et al. in 1956.
3. The Packed LC Column
(22)4. The Open Tubular LC Column
(23)
It should be noted that all the equations assume that the mobile phase
is incompressible which will not be true for equations (23) and (24). It
follows that equations (23) and (24) will require modification in order
to be applicable to practical situations.
Effect of Mobile Phase Compressibility On the HETP Equation for a
Packed GC Column
As the pressure falls along the column length, the velocity changes
and, as the solute diffusivity depends on the pressure, the diffusivity of
the solute will also change. The multi-path term, which contains no
velocity or gas pressure dependent parameters, will be unaffected and
the expression that describes it the same. The other terms in the HETP
equation, however, all contain parameters that are affected by gas
pressure (solute diffusivity and mobile phase velocity) and, therefore,
need to be modified to accommodate the compressibility of the mobile
phase.
Reiterating the HETP equation for a packed column,
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where f1(k") = and f2(k") =
Consider a point (x) along the column,
The HETP equation, as derived by Van Deemter, is seen to apply only
to a particular point distance (x) from the inlet of the column where the
pressure is constant.
Now, applying the gas laws Px u x = Pou o or
where (Px) is the pressure at point (x) along the column,
(ux) is the linear velocity of the mobile phase at point (x),
(Po) is the pressure at the column exit,
and (uo) is the linear velocity of the mobile phase at the column
exit.
Now from the kinetic theory of gases, it can be shown that thediffusivity of a solute in a gas is inversely proportional to the pressure.
Thus, DxPx = DoPo or
where (Do) is the solute diffusivity at the end of the column at (Po)
and (Dx) is the solute diffusivity at point (x) and pressure (Px)
Thus, and
Substituting for and in the HETP equation,
H x = 2 d p +2 D m ( o )
u o+
f1 ( k " ) d p2
D m ( o )u o +
f 2 ( k " ) d f2 P 0
D S P xu o
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It is now seen that if the mobile phase velocity is taken as that at the
column outlet, only the resistance to the mass transfer term for the
stationary phase is position dependent. All the other terms can be used
as developed by Van Deemter, providing the diffusivities are also
measured at the outlet pressure (atmospheric).
The resistance to the mass transfer term for the stationary phase must
be considered in isolation. The experimentally observed plate height
(variance per unit length) resulting from a particular dispersion process[e.g., (hs), the resistance to mass transfer in the stationary phase] will
be the sum of the local plate height contributions (h'); i.e.,
Consequently, substituting for (h') the expression for the resistance to
mass transfer in the stationary phase will be,
or (24)
Now, it can be shown that, (see equation 23 Book 6),
or (25)
Substituting for (Px) from equation (25) in equation (24),
(26)
Let w =
Then or
Furthermore, when x=0, then and when w = L, then .
Substituting for
and (dx) in equation (26) and inserting the new limits
and integrating,
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or
Thus, (27)
Thus, the complete HETP equation for a packed GC column, that takes
into account the compressibility of the carrier gas, will be
H = 2 d p +2 D m ( o )
u o+
f1 ( k " ) d p2
D m ( o )u o + 2
f 2 ( k " ) d f2
D S + 1( )u o (28)
Now from D'Arcy's Law
or
Thus,
Integrating from x=0 to x = L and Px = Pi to Po,
or
Solving for (), (29)
Substituting for () in equation (27) from equation (29),
Thus the HETP equation given by equation (28) becomes
H = 2 d p +2 D m ( o )
u o+
f1 ( k " ) d p2
D m ( o )u o + 2
f2 ( k " ) d f2
D Su 0 L
K P o+ 1
0 . 5
+ 1
u o(30)
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Equation (30) gives the variance per unit length of a GC column in
terms of the outlet pressure (atmospheric); the outlet velocity; and
physical and physicochemical properties of the column, packing, and
phases and is independent of the inlet pressure. However, equation (28)
is the recommended form for HETP measurements as the inlet pressureof a column is usually known, (and consequently (), the inlet/outletpressure ratio is also known) and the equation is less complex and
easier to use. The important aspect of this development is that the
resistance to mass transfer in the stationary phase is seen to be a
function of the inlet-outlet pressure ratio ().
Regrettably, the average velocity is the variable that is almost
universally used in constructing HETP curves in both GC and LC. This
is largely because it is simple to calculate from the ratio of the column
length to the dead time. Unfortunately, in GC, the use of the average
velocity provides very erroneous data and, for accurate column
evaluation and column design, the exit velocity must be employed
together in conjunction with the inlet-outlet pressure ratio.
An example of the errors that can occur from the use of the average
velocity, as opposed to the exitvelocity, is shown in figure 9 from data
obtained for a capillary column.
H E T P C u r v e E m p l o y i n gt h e E x i t V e l o c i t y
H E T P C u r v e E m p l o y i n gt h e A v e r a g e V e l o c i t y
M o b i l e P h a s e V e l o c i t y ( c m / s e c . )
P
la
te
H
eig
h
t
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Figure 9. HETP Curves for the Same Column and Solute Using the
Average Mobile Phase Velocity and the Exit Velocity
The two curves are clearly quite different and, if the results are to befitted to the HETP equation, only the data obtained using the exit
velocity will give meaningful values for the exclusive dispersion
processes. This problem is further emphasized in the graphs shown in
figure 10. In figure 10, the individual contributions from the different
dispersion processes are obtained by deconvoluting the HETP curve
obtained using the average velocity data.
It is seen that using the average velocitydata, the extracted value for
the multi-path term is negative, which is physically impossible (for acapillary column should be zero or very close to zero). In contrast, the
values obtained from data involving the exit velocity give small
positive, but realistic values for the multi-path term.
In all aspects of column evaluation and column design in GC, the
compressibility of the mobile phase must be taken into account or
serious errors will be incurred.
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L o n g i t u d i n a l D i f f u s i o n B / u
H E T P C u r v e ( H )
R e s i s t a n c e t oM a s s T r a n s f e r C u
0
M u l t i - p a t h T e r m A
A v e r a g e V e l o c i t y ( c m / s e c . )
H
(cm
)
Figure 10. De-Convolution of the HETP Curve Obtained Using the
Average Mobile Phase Velocity
The Van Deemter Equation
The Van Deemter equation (9) was derived as long ago as 1956 and
was the first rate equation to be developed. There are, however, a
number of alternative rate equations that have been reported, but when
subjected to experimental test, the Van Deemter equation has been
shown to be the most appropriate equation for the accurate prediction
of dispersion in chromatographic systems. The Van Deemter equation
is particularly pertinent at mobile phase velocities around the optimum
velocity (a concept that will shortly be explained). Consequently, as all
columns should be operated at, or close to, the optimum velocity formaximum efficiency, the Van Deemter equation is particularly
important in column design. Restating the Van Deemter equation,
where f1(k") = and f2(k") =
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Note, this equation ignores the second order effect of any longitudinal
diffusion that might be present in the stationary phase. In fact, in the
original form, the equation was introduced by Van Deemterfor packed
GCcolumns and consequently, the longitudinal diffusion term for the
liquid phase was not included and the function 2 Dmu
1+ k' , was
replaced by,2 Dm
u. This was because the diffusivity of the solute in a
gas is four to five orders of magnitude greater than in a liquid.
Thus, in the expression for longitudinal diffusion,
the second function would not be significant.
In addition, Van Deemter considered the resistance to mass transfer in
the mobile phase to be negligible. This was because the eddies that
form between the particles causes a turbulence or secondary flow that
greatly increases the diffusivity of the solute between the pores. As a
result, the function,, was also not included. Consequently, the equation
actually developed by Van Deemter took the form,
The form taken by f2(k') was considered by Van Deemter to be,
and thus, the complete HETP equation became,
(31)
Equation (31), however, was developed for a GC column and in the
case of an LC column, the resistance to mass transfer in the mobile
phase should be included. Van Deemter et al. did not derive an
expression for f1(k') for the mobile phase but Purnell (10) suggested
that the function of (k'), employed by Golay (8) for the resistance to
mass transfer in the mobile phase in his rate equation for capillaryThis eBook is protected by Copyright law and International Treaties. All rights are reserved. This book is covered by an End User Licensee
Agreement (EULA). The full EULA may be seen athttp://www.library4science.com/eula.html.
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columns, would also be appropriate for a packed column. The form of
f1(k') derived by Golay was as follows,
Thus, Van Deemter's equation for LC becomes,
(32)
Equation (32 ) can put in a simplified form as follows,
(33)
where, A=2d p, B=2 D m and
Equation (33) is a hyperbolic function which has a minimum value of
(H) for a particular value of (u). Thus, a maximum efficiency will
obtained at a particular linear mobile phase velocity.
An example of an HETP curve obtained in practice showing this
hyperbolic relationship is given in figure 11.
-0.000 0.100 0.200 0.300 0.400 0.5000.600
u ( c m / s e c )
-0.000
0.001
0.002
0.003
C u r v e F i t
M u l t i p a t h T e r m
R e s i s t a n c e t oM a s s T r a n s f e r
L o n g i t u d i n a lD i f f u s i o n
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Figure 11. HETP Curve for Hexamethylbenzene
The HETP curve is the result of a curve fitting procedure to the
experimental points shown. The column was 25 cm long, 9 mm in
diameter and packed with 8.5 micron (nominal 10 micron) Partisil
silica gel. The mobile phase was a solution of 4.8%w/v ethyl acetate in
n-decane. The hyperbolic form of the curve is confirmed, the minimum
is clearly indicated and the fit of the points to the curve is good. From
the curve fitting procedure the values of the Van Deemter constants
could be determined and the separate contributions to the curve from
the multipath dispersion, longitudinal dispersion and the resistance to
mass transfer calculated and included in the figure.
It is seen that the major contribution to dispersion at the optimum
velocity (where the value of (H) is a minimum) is the multipath effect.
Only at much lower velocities, does the longitudinal diffusion effect
become significant. Conversely, the mobile phase velocity must be
increased to about 0.2 cm/sec before the dispersion due to the
resistance to mass transfer begins to become relatively significant
(compared to that of the multipath effect).
The values for the Van Deemter constants were found to be,
A=0.00117B=0.0000175 cm2/sec
and C=0.00250 sec.
If the mean particle size was 0.00085 cm, then as, A = 2 dp
Then, 0.00117 = 2 0.00085 or, = 0.69
Giddings (11) determined theoretically that, for a well packed column
() should take a value of about 0.5 and thus the column used was
reasonably well packed.In a similar manner, as B = 2Dm
Then, 0.0000175 = 2gDm
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Katz et al (12) determined the diffusivity of hexamethylbenzene in
4.83%w/v ethyl acetate in n-decane and found it to be 1.17x10-5
cm2/sec,
Consequently, = 0.747
Giddings (11) also determined that, for a well packed column, ()should be about 0.6 so again the dispersion from longitudinal diffusion
as measured. confirms that the column was reasonably well packed.
For a packed column, the particle size has a profound effect on the
minimum value of the HETP of a column and thus the maximum
efficiency attainable. It would also indicate that the highest column
efficiency would be obtained from the smallest particles. However, this
assumes that an unlimited pressure is available and the apparatus cantolerate such pressures. Within practical limits of pressure, the smaller
the particle diameter, the smaller will be the minimum HETP and thus,
the larger the number of plates per unit length obtainable from the
column. However, the total number of theoretical plates that can be
obtained, will depend on the length of the column which, in turn, must
take into account the available inlet pressure.
The optimum mobile phase velocity can be obtained by differentiating
equation (33) with respect to (u) and equating to zero, thus,
and
Equating to zerodH
du= 0 and consequently,
B
u2
+ C = 0
Thus, (34)
Substituting for (B) and (C),
and letting Ds = Dm,
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(35)
It is seen from equation (35) that the optimum velocity is, directly
proportional to the diffusivity of the solute in the mobile phase. To a
lesser extent it also appears to be inversely dependent on the particlediameter of the packing and the film thickness of the stationary phase.
The film thickness of the stationary phase is determined by the physical
form of the packing, that is, in the case of silica gel, the nature of the
surface and in the case of a reverse phase, on the bonding chemistry.
Now, if it is assumed that df > 1, that is, for well retained peaks, and taking
() as 0.6
u o p t = D md p
4 . 4 2 [ ] 0 . 5 2 . 1 D md p
1 . 6 3 D md p
(36).
Under these circumstances, it is seen that the optimum velocity is
directly proportional to the solute diffusivity in the mobile phase and
inversely proportional to the particle diameter of the packing. The
quality of the packing, also plays some part, but to a very less
significant extent. It is now possible to determine the factors that
control the magnitude of Hmin. Substituting the function for uopt from
equation (34) in equation (33) an expression for Hmin is obtained.
and (37)
Substituting for A, B, and C,
(38)
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Noting that Ds= Dm, and simplifying,
(39)
Again, assuming that, df
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or, n P d p
2
2 . 4 D m (43)
It is seen from equation (43) that, if an LC column is operated at its
optimum linear velocity, the maximum efficiency obtainable for well
retained peaks will be directly proportional to the inlet pressure
available (P) and the square of the particle diameter of the packing.
Thus, the larger the particle diameter, the greater efficiency attainable
at a given pressure. This is because, as the particle diameter is
increased the column permeability is also increased allowing a longer
column to be used. The permeability increases as the square of the
particle diameter but the variance per unit length only increases
linearly with the particle diameter. Thus, doubling the particle diameterwill allow a column four times the length to be used but the number of
plates per unit length will be halved. Consequently, the column
efficiency will be increased by a factor of two. It is also seen that the
higher efficiencies will be obtained with mobile phases of low
viscosity and for solutes of low diffusivity. Solvent viscosity and solute
diffusivity tend to be inversely proportional to each other and so the
sensitivity of the maximum obtainable efficiency to either solvent
viscosity or solute diffusivity will generally not be large. The
approximate length of a column that will provide the maximum column
efficiency when operated at optimum velocity is given by, l = nHmin.
Thus, =0 . 6 2 P d p
3
D m (44)
It is seen that the column length varies inversely as the product of the
solute diffusivity in the mobile phase and the mobile phase viscosity in
much the same way as the column efficiency does when operating atthe optimum velocity. As would be expected the column length is
directly proportional to the inlet pressure but, less obviously is also
proportional to the cube of the particle diameter.
The analysis time for a solute mixture in which the last peak is eluted at
a capacity ratio of k'F is given by,
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t = (1 + k'F )t 0 = (1 + k'F )l
u opt
Substituting for (uopt) and (l) from equations (36) and (44),
or, t = ( 1 + k ' F )0 . 4 9 P d p
4
D m2
(45)
It is seen from equation (45) that the analysis time is proportional to the
fourth power of the particle diameter and inversely proportional to the
square of the diffusivity in the mobile phase. In a similar manner to
column length, the analysis time is also directly proportional to the
applied inlet pressure and inversely proportional to the mobile phase
viscosity.
Summarizing, if a column is operated at its optimum velocity and the
solute concerned is eluted at a relatively high k' value, and assuming
the film thickness of the stationary phase is small compared with the
particle diameter (a condition that is met in almost all LC separations)
then,
u o p t 1 . 2 6 D m
dp
(36)
Hmin. 1.48dp (46)
n P d p
2
2 . 4 D m (43)
l 0 . 6 1 7 P d p
3
D m (44)
t (1+ k'F )0 .38 Pd
p
4
Dm
2
(45)
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As already stated, these equations are insufficiently precise to be used
for accurate column design but, they can give a general indication of
the more important performance specifications that could be expected
from an approximately optimized chromatographic system.
It would be of interest to use the equations to calculate the maximum
efficiency, column length and analysis time that would be obtained
from columns packed with particles of different diameter under
conditions that commonly occur in LC analyses.
The diffusivity of solutes having molecular weights ranging from about
60 to 600 vary from about 1x10-5 to 4x10-5 cm2 /sec.(13) Thus, an
average value of 2x10-5 cm2 /sec will be taken in the following
calculations. In a similar way a typical viscosity value for the mobile
phase will be assumed as that for acetonitrile (14), i.e. 0.375x10-2
poises. The inlet pressure taken will be 3,000 p.s.i. or about 200
atmospheres. Many LC pumps available today will operate at 6,000
p.s.i. or even 10,000 p.s.i., however, it is not the pump that determines
the average operating pressure of the chromatograph, but the sample
valve.
Sample valves can, for a limited time, operate very satisfactorily at
very high pressures but their lifetime at maximum pressure issignificantly reduced. Most valves, designed for high pressure
operation will have extensive lifetimes when operated at 3,000 p.s.i.
and so this is the pressure that will be employed in the using the above
equations. The value assumed for the d'Arcy constant,() is 35 when(P) is measured in p.s.i. and has been determined experimentally (14).
The capacity factor of the last eluted peak was taken as 5 for
calculating the elution time. Employing the above values, equation (16)
was used to calculate maximum efficiency attainable for columns
packed with particles of different diameters. The results obtained are
shown in figure 12. It is seen from figure 12 that changing the particle
diameter from 1 to 20 micron results in an efficiency change from
about 3500 theoretical plates to nearly 1.5 million theoretical plates
and furthermore, this very high efficiency is achieved at an inlet
pressure of only 3000 p.s.i..This eBook is protected by Copyright law and International Treaties. All rights are reserved. This book is covered by an End User Licensee
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0 10 20 30
3
4
5
6
7
P a r t i c l e D i a m e t e r ( m i c r o n )
Figure 12. Graph of Log Maximum Efficiency against Particle
Diameter
It is also seen that the maximum available efficiency increases as the
particle diameter increases. This is because, as already discussed, if the
pressure is limited, in order to increase the column length to provide
more theoretical plates, the permeability of the column must be
increased to allow the optimum mobile phase velocity to be realized. It
is possible to increase the inlet pressure to some extent, but ultimately
the pressure will be limited and the effect of particle diameter will be
the same but at higher efficiency levels. The column lengths necessary
to achieve these efficiencies can be calculated employing equation
(44). The results obtained are shown as curves relating maximum
column length to particle diameter in figure 13.
It is seen from