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Proc Natl Acad Sci U S A. Apr 30, 2002; 99(9): 5816–5821.
PMCID: PMC122859
Chemistry

Determination of causal connectivities of species in reaction networks

Abstract

We present an approach to the determination of causal connectivities and part of the kinetics of complex reaction systems. Our approach is based on analytical and computational methods for studying the effects of a pulse change of concentration of a chemical species in a reaction network, either at equilibrium or in a nonequilibrium stationary state. Such disturbances generally propagate through a few species, depending on the values of the kinetic coefficients, before being broadened and dissipated. This short range gives a local probe of the kinetics and connectivity of the reaction network. The range of propagation also indicates species to perturb in further experiments. From piecing together these local connectivities, the global structure of the network can be constructed. The experimental design allows deduction of both reaction orders and rate constants in many cases. An example of the usefulness of the approach is illustrated on a model of a part of glycolysis.

Standard methods used for the study of the structure of reaction networks include determination of the stoichiometry and kinetics of individual steps followed by hypothesizing reaction mechanisms and testing them against such measurements; perturbations of reaction systems with first-order kinetics to determine the constant rate matrix (1); and introduction of radioactive tracers to determine reaction connectivities (2). In addition, several approaches are used to infer causal relationships in genetic networks; however, most of these techniques are applicable only to Boolean networks (38). Our work has taken several different approaches to this problem in nonequilibrium systems (915), all based on not dissecting the system but maintaining all interactions. Using fluctuating input concentrations, we have shown how correlations among species measured in the entire system may be used to construct distances among species and from this infer information on the reaction pathway (11, 12). This correlation metric construction gives a hierarchy of influence in a system and identifies weakly coupled subsystems; causal connectivities can be obtained with more difficulty. The methods outlined in the present paper give causal reaction connectivities of measured species and regulatory features of a reaction network through analyses of responses of a system to pulse perturbations. For these techniques, the concentrations of species affected by a given pulse need to be measured in time. The measurement resolution required, both in concentration and time, depends on the stationary state concentration values, the rates of reaction, and the connectivity of the reaction network. However, adequate estimates of concentration detection levels may be based on stationary state values, and estimates of time resolution levels may be based on the time of appearance of extrema after a pulse perturbation. Typically, a modest number of time measurements, often 10 or fewer, is sufficient to approximate extrema locations and values. From these measurements, both reaction orders and rate constants of an empirical rate equation may be deduced in many cases. The global structure of the reaction network is obtained by piecing together these local connectivities. We start with straightforward examples to show the simplicity of the approach and then indicate the applicability to complicated cases. An example of the usefulness of the approach is illustrated on a model of a part of glycolysis.

The number of species that need to be pulsed to deduce the causal connectivities of the species, and hence the reaction pathway, depends on the complexity of the reaction system; we do not address the issue of rules applicable to this point. At most, all the species of the system need to be pulsed, which will lead to all connectivities, but frequently fewer than all are necessary. We illustrate in the Appendix how connectivity may be obtained by using few perturbations in a simple example.

Method and Theory

The application of the impulse perturbation method to a reaction network consists of changing the concentration of a given species over a short time and then observing the concentration responses X induced in it and other species. A plot of the deviation in concentration from the stationary state value, XXs, against time shows that for unbranched chains of reactions, the (first) extrema in the concentration of species are ordered along the time axis with decreasing amplitude according to the number of reaction steps separating that species from the initially perturbed species. Pulses propagate strongly, i.e., with large amplitude, in the direction of net reaction velocity and weakly in the reverse direction. As an example, we consider the case of an unbranched chain of reversible first-order reactions:

equation M1
1

For first-order reactions, it is convenient to study the relative change in concentration u = (XXs) = Xs as a function of time, u(t). These reduced variables exhibit relatively simple relations at extrema. Equating the time derivative of ui(t) to zero at the time of an occurrence of an extrema ti, we obtain a relation between the extremum value ui(ti) and the values of the relative concentrations of other species uji(ti). In the following, we often abbreviate the extremum value as uequation M2 and omit explicit reference to time ti. From the deterministic kinetic equations for Eq. 1, we obtain

equation M3
2

where the coefficient α is less than one,

equation M4
3

jf = ki−1Xequation M5 is the steady state forward flow into Xi; and jT = jf + jr is the total flow into Xi. This relation shows that a maximum in ui occurs between the curves for the preceding and succeeding species; i.e., in addition to time ordering of extrema, the values at maxima of (relative deviations of) species are also ordered according to the number of reaction steps separating that species from the initially perturbed species. The usefulness of these relations follows from their geometric interpretation and independence from rate values. Measurements to investigate connectivity of species through reactions need only determine times of occurrences of extrema and concentration values of species at them. Fig. Fig.11a shows the propagation of a pulse following a pulse perturbation of the first species X1 in the chain of reactions. Using relative deviations of concentrations, we verify that maxima, as well as values at maxima, are ordered according to the number of reaction steps separating that species from the initially perturbed species. The effect of perturbing a species in the middle of the chain is shown in Fig. Fig.11b. In this case, the pulse propagates with large amplitude in the direction of the overall reaction velocity and weakly in the opposite direction. For segments of systems in which there is not a large net reaction velocity, e.g., for subsystems close to equilibrium, a pulse perturbation induces extrema in neighboring species that are similar in magnitude: a pulse propagates equally in both directions away from the perturbation source.

Figure 1
Plots of the relative deviation in concentration from the stationary state versus time for all the species of the mechanism in Eq. 1. The maxima are ordered according to the number of reaction steps separating that species from the initially perturbed ...

More complicated mechanisms are studied through an analysis of times and values of extrema in concentration changes of species. These values give information about local connectivities and kinetics (e.g., feedback, higher-order kinetics). Several observations, which often hold, may be used as guidelines in the initial construction of connectivities of species in a reaction network. (i) The time of an extremum increases as the number of reaction steps separating that species from the initially perturbed species increases, unless some species act as effectors in distant reactions. (ii) Conversely, the initial curves of concentration changes of a species with time approach the time axis as the number of reaction steps separating that species from the initially perturbed species increases (in the absence of effectors). (iii) Species that are directly connected through reactions to the initially perturbed species exhibit nonzero initial slopes. (iv) Species that are not directly connected through reactions to the initially perturbed species exhibit zero initial slopes. (v) All responses are positive deviations from the stationary state unless there is a feedback, feedforward, or higher-order (>1) kinetic step. (vi) For short times, prior to the exit of material from the pulse to the surroundings of the reaction system, the concentration change of the pulse is conserved: the sum of deviations of concentrations (weighted by stoichiometric coefficients) must be constant and equal to the change in concentration of the initial pulse. This property is useful in confirming that all species produced from the pulse through reactions have been detected and can help in determining correct stoichiometric coefficients. (vii) When it is possible to identify the rate expressions for reaction steps, then kinetic constants may be estimated from the values of the concentrations of species at an extremum. In the above example, the value of α, Eq. 3, may be estimated from extrema, which gives the ratio ki−1/ki.

We have investigated the effects of some geometrical arrangements and rate expressions on the conditions for extrema. The geometries considered include (i) straight chains, (ii) branched chains, i.e., several chains converging and diverging from a given species, (iii) positive and negative feedback and feedforward, and (iv) a cycle of reactions. The rate expressions treated include: (i) first- and second-order kinetics, (ii) generalized mass-action kinetics (for small perturbations), and (iii) uni-uni enzyme catalyzed reactions (Michaelis–Menten). The analytic solutions for these simplify considerably for the case of irreversible reactions.

First-Order Kinetics.

We consider a set of reactions that may be described by first-order or pseudo-first-order kinetics; e.g., reversible Michaelis–Menten kinetics in which the substrate concentration is low. Specifically, the reactions either produce or consume a species X:

equation M6
4

Then the rate expression for X is

equation M7
5

The evolution of the relative deviation from the stationary state, u = (X  Xs) = Xs, may be written

equation M8
6

where αi = ji/jT, ji = kiXequation M9, and jT = ∑ji. We note that the sum of coefficients is equal to one: ∑αi = 1. An extremum in u occurs when the above derivative with respect to time is zero, which for this system results in the expression:

equation M10
7

This abbreviated form for the relation between values of variables at an extremum of u omits explicit inclusion of the time variable; implicit in this expression is the evaluation of all variables at time t* at which du/dt = 0.

From this expression, we have the result that an extremum u* occurs within (the convex hull of) the curves ui for the species that produce X. For example, in the case of a chain of irreversible reactions X1XX2, the extremum u* occurs on u1; the curve for the species that produces X. Another example is the case of irreversible reactions in which two species, X1 and X2, separately produce X; and X produces one product X3. Then u* occurs between the curves for the species that produce X, u1, and u2, and at such a point the coefficients sum to one: α1 + α2 = 1.

Fig. Fig.22 shows a diagram of converging chains of irreversible first-order reactions. Perturbation of species X1 causes a pulse to propagate through the sequence X2; X3; X4; X5, Fig. Fig.33a; perturbation of species X8 causes the pulse to propagate through the sequence X7; X6; X3; X4; X5, Fig. Fig.33b. In each of these figures, we note that aside from the branch species X3, the maximum value (of the relative deviation) of a species occurs on the curve for the species that produces it. For the branch species, the maximum value of u3 is equal to αi ui, where i is 2 or 6, depending on whether the pulse propagate through species X2 or X6, i.e., whether X1 or X8 is perturbed. The sum of the coefficients α2 + α6 is equal to one and is a useful check on the correct number of converging chains at X3. These relations may be extended to networks of nearly irreversible reactions, where they hold to within a correction that is the order of the reverse rate divided by the forward rate.

Figure 2
Chemical reaction mechanism for converging chains of irreversible first-order reactions. The rates of production of species X1 and X8 are held constant at 0.1 and 0.5, respectively. [Xi]0 denotes the stationary state concentration of species ...
Figure 3
Plots of relative deviation in concentration versus time for species of the mechanism in Fig. Fig.2.2. In a, a perturbation of the concentration of species X1 causes a pulse to propagate through the sequence X2; X3; X4; X5; in b, perturbation ...

Cyclic reaction systems may be investigated by using the above methods. Such systems are composed of chains of reactions that form a closed loop; inputs and outputs are branch points of the loop. Using Eq. 7, the linear and branch points of the system may be identified through appropriate perturbations. Another class of systems for which the above methods and results are directly applicable is those in which radioactive tracer species are introduced. If a tracer is added so that the total concentration of the species is constant, then the response of the tracer obeys first-order kinetics.

Generalized Mass-Action Kinetics.

The propagation of pulses, and in particular the conditions for extrema, may also be described for higher-order reaction kinetics.

For the case of two different species reacting, we take the following reaction scheme:

equation image
8

The condition for an extremum in one of the species ub involved in the bimolecular reaction may easily be derived. For small reverse velocities, j−1/jT [double less-than sign] 1; the condition reduces to

equation M11
9

where

equation M12
10

and j−1 = k−1Xequation M13, jT = jb + j1 = kbXequation M14 + k1Xequation M15Xequation M16. If the second-order reaction rate is much greater than the rate of the other reaction that destroys Xb, then we have jb/j1 [double less-than sign] 1, and Eq. 9 reduces to u*b = −ua/(1 + ua). The approximate condition for an extremum in the product u2, for small reverse rate coefficient jb/j1 [double less-than sign] 1

equation M17
11

To illustrate an application of these conditions, we consider an impulse change of concentration of species Xa in Eq. 8. Following this perturbation, the concentration of species Xb decreases below the stationary state value and reaches a minimum value given by Eq. 9. The concentration of the product of the reaction increases and reaches a maximum value given by Eq. 11. For small perturbations, the maximum value u*2 is the sum of ua and ub.

Generalized mass-action kinetics may be treated similarly. We consider the case in which the creation and consumption of a species X1 are each single reactions with power rate laws (we assume the reverse rates of these reactions are small):

equation M18
12

The sets of species that produce X1; (Xa, Xb, … , Xl); and the set of products, (X1, X2, … , Xn); are not necessarily disjoint. These types of rate equations, called S-systems, have been applied to the analysis of biochemical pathways and genetic networks (16). Then for small deviations from the stationary state, the equation may be linearized, which leads to the following condition at an extremum in u1 (du1/dt = 0)

equation M19
13

That is, as in the case of irreversible first- and second-order kinetics, at an extremum the values of the reduced variables are linearly related with coefficients determined only by the exponents η. For these and similar systems, the exponents η may be determined through experiments that probe the effects of perturbing different species that are involved in reactions that create X1.

We illustrate the application of this relation by using a sequence of first- and second-order reactions given in Fig. Fig.4.4. In this example, where a single species is produced and destroyed at each reaction step, the above relation simplifies to u*1 ≈ (ηa1)ua. An impulse perturbation of X1 results in the responses shown in Fig. Fig.5.5. Connectivities between species are reflected in the times of extrema of the relative deviations: u2 follows u1, … , u8 follows u7. The relations between the variables at extrema give ratios of exponents. For example, X2 is produced through a first-order reaction involving X1 and consumed through a second-order reaction of X2. This results in the relation u*2 ≈ (η12)u1 = (1/2)u1 at an extremum in X2; i.e., the order of the second reaction is determined from the extremum relation. The other relations are similarly determined at extrema of Fig. Fig.44 and are u*3 ≈ 2u2, u*6 ≈ (1/2)u5, and u*7 ≈ 2u6. Using these relations along with other information, such as initial rate studies, the rate coefficients ki may be determined.

Figure 4
Chemical reaction mechanism of a linear chain of coupled first- and second-order reactions. The order of a reaction is given by the stoichiometry.
Figure 5
Plots of relative deviation in concentration versus time for species of the mechanism in Fig. Fig.4.4. A pulse perturbation of the concentration of species X1 results in the responses shown. The pulse propagates through the chain with maxima of ...

Feedback and Feedforward.

Feedback and feedforward effects arise in chemical reaction networks from a variety of mechanisms. The rate of a reaction may be either increased or decreased by an effector species not directly involved in the reaction; the location of this effector species in the network may either precede (feedforward) or succeed (feedback) the reaction. A general mechanism may be treated by linearizing the equations about a stationary state. For these cases, absolute deviations from the stationary state are more useful than relative deviations, because the species directly affected by the reaction show symmetric deviations. We consider an effector species Xeff either promoting or inhibiting the reaction XiXi+1, and all reverse processes are assumed negligible. We assume a general rate function f(Xi; Xeff) for the feedforward or feedback that has nonzero derivatives with respect to Xi and Xeff at the stationary state. Then the linearized rate equations are

equation M20
14

equation M21
15

where ΔXi denotes the deviation in concentration of species Xi from the stationary state value and ai = [partial differential]f/[partial differential]Xi, aeff = [partial differential]f/[partial differential]Xeff. If aeff > 0 (aeff < 0), then Xeff acts as an activator (inhibitor) of the reaction. The effector species Xeff and its influence on the reaction may be identified through a (direct or indirect) perturbation of the concentration of Xeff. After such a perturbation, for short times such that changes in Xi; Xi−1, and Xi+1 are small in comparison to ΔXeff, deviations in species Xi and Xi+1 are mirror images about the time axis:

equation M22
16

[Assuming ΔXeff and the coefficients a are O (1) and that ΔXit)/ΔXf is small O (epsilon), then Δt = O (epsilon) for this relation to hold.] The extrema are ordered with the extremum of ΔXi+1 occurring before that of ΔXi, independent of the sign of aeff (assuming that Xeffdoes not influence Xi−1 significantly, e.g., Xeff does not directly produce Xi−1). This may be shown as follows: if aeff > 0, then ai ΔXi + aeffΔXeff starts out positive, which implies a consumption of Xi by Eq. 15, and decreases to zero at the minimum of ΔXi; Eq. 15 (the influence of Xi−1 is negligible if it is not influenced directly by Xeff). According to Eq. 16, ΔXi+1 initially increases, because ai ΔXi + aeff ΔXeff > 0, and reaches a maximum value at the crossing of the curves ai+1 ΔXi+1 and ai ΔXi + aeff ΔXeff which occurs before the minimum of ΔXi (at ai ΔXi + aeff ΔXeff = 0). Similarly, if aeff < 0; then ai ΔXi + aeff ΔXeff starts out negative and increases to zero at the maximum of ΔXi; following the previous argument, the minimum of ΔXi+1 occurs before the maximum of ΔXi. This ordering of extrema allows the identification of the direction of the net reaction velocity XiXi+1.

An example of a system with positive feedback is shown in Fig. Fig.6.6. The associated rate equations are integrated for a perturbation in concentration of X1 and X7; the absolute deviation of concentration from the stationary state is given in Fig. Fig.77 a and b, respectively. Fig. Fig.77a shows maxima of species occurring in the order of species in the chain of reactions X1X8. Species X3 falls below the stationary state value, which indicates a possible feedback effect from one of the later species. A trial perturbation of X7, Fig. Fig.77b, shows that X3 and X4 are mirror images about the time axis for short times, and their initial slopes are nonzero. These observations indicate that X7 activates the reaction from X3 to X4 (the peak of X4 occurs before that of X3, implying that X3 precedes X4 in the reaction sequence).

Figure 6
Chemical reaction mechanism illustrating positive feedback in a linear chain of irreversible first-order reactions. The rate of production of species X1 is held constant at vf.
Figure 7
Plots of deviation in concentration ΔX from the stationary state value versus time for the species of the mechanism in Fig. Fig.6.6. In a, a perturbation of the concentration of species X1 causes a pulse to propagate through the linear ...

Enzyme-Catalyzed Reactions.

Many segments of biochemical pathways may be modeled as unbranched chains consisting of enzyme-catalyzed reactions. We concentrate on a chain in which the kinetics are described by the irreversible Michaelis–Menten equation:

equation M23
17

The rate of the relative deviation of S2 is given by

equation M24
18

For small deviations from the stationary state, we linearize the equations, use the stationary state condition for the relation between Sequation M25 and Sequation M26, and obtain the following expression for an extremum in u2:

equation M27
19

where Km1 = (k−1 + k2)/k1; Km3 = (k−2 + k3)/k2: We see that, unlike the case of first-order reactions, the value of u*2 may be greater or less than u1. If the concentrations of the substrates are much smaller than the corresponding Michaelis constants, i.e., Sequation M28/Km1 [double less-than sign] 1; Sequation M29/Km3 [double less-than sign] 1, then kinetics reduce to first-order, and the above relation becomes that for the case of irreversible first-order kinetics, u*2 = u1.

An Example: The Glycolytic Pathway

We present an application of some of the methods outlined above to a model of the glycolytic pathway. The model we use includes many of the known activations and inhibitions of enzymes by metabolites, Fig. Fig.8.8. The HKase reaction is assumed to operate at constant rate, which neglects the influence of ATP and glucose 6-phosphate. The concentrations of glucose, lactic acid, and the total adenine nucleotide pool are kept constant; the AKase reaction is assumed to be at equilibrium. Prior to the application of a pulse, the system is in a nonequilibrium stationary state. We refer to ref. 17 for details concerning the assumptions and the derivation of rate equations. There are five independent variables: fructose 6-phosphate (F6P), fructose 1,6-bisphosphate (FDP), phosphoenolpyruvate (PEP), pyruvate (PYR), and ATP; in the following, we label the variables 1–5, respectively. Our parameter values are the same as those in ref. 17, except for the input rate, which we take as V = 1.5 mM/min.

Figure 8
Chemical reaction mechanism for an abbreviated model of the glycolytic pathway. The mechanism includes many of the known activations and inhibitions of enzymes by metabolites. Broken lines indicate activation [plus sign in circle] or inhibition [hyphen in circle] of enzymes ...

Fig. Fig.99 ad shows time series for the absolute deviations of species with impulse perturbations of F6P (1), FDP (2), PEP (3) and ATP (5); solutions were obtained from numerical integration of the model equations. In Fig. Fig.99a, the response to an impulse perturbation of (1) is shown. The variables exhibit extrema in the following order in time 2, 3, 4; the variable 5 exhibits both a minimum and a maximum. Variables 3 and 4 have zero initial slopes, which is consistent with their production from 2: the deviation in 2 starts at zero, which implies that the velocity of 2 into any of its products, e.g., (3, 4), is initially zero. Also, for short times, the deviations in 3 and 4 are mirror images about the time axis, which indicates that the conversion between 3 and 4 is affected by 2 (if 1 were to affect this conversion, then the initial slope of 3 and 4 would be nonzero). A separate perturbation of 4, which is not shown, does not produce a significant response in 3; therefore, it is inferred that 3 produces 4. A verification that 1 is converted to 4 is shown in Fig. Fig.1010a, where the sum of the deviations in concentrations ΔX1 + ΔX2 + (ΔX3 + ΔX4)/2 is slowly decaying in time. This indicates an approximate conservation of mass among these species. We note from this conservation that each molecule of species 2 produces two molecules of species 3, which in turn produces (one molecule of) species 4. The initial slope of 5 in Fig. Fig.99a is equal to minus that of 2, which shows that 5 is consumed in equal numbers to 2 produced. In summary, from the responses to a perturbation of 1 (and 4), we have the results: 1 produces 2, 2 produces 3, 2 activates the conversion of 3 to 4, 3 produces 4, and 5 is consumed in the conversion of 1 to 2 (with the stoichiometric ratio of species 5 to species 2 being 1:1).

Figure 9
Plots of time series for the absolute deviations in concentrations of species of the mechanism in Fig. Fig.88 with impulse perturbations of F6P (1), FDP (2), PEP (3) and ATP (5). From an analysis of the responses to these perturbations, we deduce: ...
Figure 10
Plots of time series for sums of deviations in concentrations for the species of the mechanism in Fig. Fig.8.8. In a, the concentration of species X1 is perturbed; in b, the concentration of species X3 is perturbed. Plot a shows that the sum of ...

Fig. Fig.99b shows responses to an impulse perturbation of species 2. The initial slopes of 3 and 4 are nonzero, which indicates that 2 has a direct effect on (activates) the conversion of 3 to 4; the initial effect of 2 is to activate the reaction from 3 to 4 (and slowly produce 3). The minimum in 3 precedes the maximum in 4 following a perturbation of 2, which indicates that 2 directly produces 3 and shifts the minimum of 3 (which would occur after the maximum in 4 without this direct production) to an earlier time. Species 1 does not respond to the perturbation, which shows that the conversion of 1 to 2 is highly irreversible. The initial slope of species 5 is equal to that of 4, which shows that 5 is produced at the same rate as 4 in the reaction 3 to 4. The new information from this perturbation is the production of 5 in this latter reaction.

Fig. Fig.99c shows responses to an impulse perturbation of species 3. Both 2 and 4 have nonzero initial slopes, which shows that 3 produces both 2 and 4. The small amplitude of 2 indicates that the reaction 2 to 3 is reversible. New information is also contained in the initial time series for 2 and 5: 5 is consumed at the same rate as 2 is produced, which indicates that 5 is a cosubstrate for the reverse reaction of 3 to 2. Fig. Fig.1010b shows a transient conservation of mass in species 2, 3, and 4; the initial flow is from 3 to (1/2) 2 and over a longer time from 3 to 4.

Fig. Fig.99d shows responses to an impulse perturbation of species 5. The minus signs in the figure denote reflection of the deviations about the time axis. The increase of 1 and decrease of 2 indicate that 5 inhibits the reaction 1 to 2, without affecting the rate of 2 to 3. The opposite rates of 3 and 4 indicate that 5 also inhibits the conversion of 3 to 4.

From the above analysis of the propagation of pulses in the glycolytic pathway, we may construct the reaction scheme shown in Fig. Fig.11.11. This diagram captures the topology of the reaction network and many of the effectors. Further studies of the adenine nucleotides would help determine the role of the other effector (AMP) and other substrates, such as ADP, for each reaction.

Figure 11
A simplified mechanism constructed from the analysis of Figs. Figs.99 and and10.10. This diagram captures the topology of the reaction network in Fig. Fig.88 and many of the effectors.

Discussion

From an analysis of responses of reaction systems to pulse perturbations in concentrations of chemical species (applied to stationary state), we are able to construct the dominant kinetic structure of reaction networks. The level of information obtained depends on the number of species that are accessible to measurement and external perturbation. While correct deductions about the order of a particular reaction necessitates all involved species be identified and measured, much of the network structure can be obtained with less information. For example, in some biochemical systems, the kinetics of reactions may be treated as first-order or pseudo first-order; in these cases, identification of ordering of species in linear chains of reactions and branch points follows from analysis of extrema following appropriate perturbations. In these systems, it is also possible to determine the location of species that have not been measured in the network and the number of chains converging or diverging from a branch point from locations of extrema and sums of relative fluxes, respectively. Blind tests of the methods presented here are needed. These studies will be performed on realistic models of biological pathways and should help determine the numbers of measurements needed to construct networks of a given level of complexity.

Acknowledgments

This work was supported in part by the National Science Foundation.

Appendix

Much can be learned, by simple deduction, from measuring the responses to a pulse perturbation of a given species in a reaction mechanism. Consider the following case: a flow from the main branch into a side branch given in Fig. Fig.12.12. Perturbations of only three chemical species, X1, X2, X6, and calculations of the responses of the other species suffice to deduce the causal connectivities of the species and the reaction mechanism.

Figure 12

An external file that holds a picture, illustration, etc.
Object name is pq0620496012.jpg

Chemical reaction mechanism for diverging chains of first-order reactions. The rates of production of species X1 are held constant at 0.1.

References

1. Wei J, Prater J D. Advances in Catalysis. Vol. 13. New York: Academic; 1962. pp. 204–390.
2. Boudart M. Kinetics of Chemical Processes. Englewood Cliffs, NJ: Prentice-Hall; 1968.
3. Liang S, Fuhrman S, Simogyi R. Pacific Symposium on Biocomputing. 1998;3:18–29. [PubMed]
4. Weaver D C, Workman C T, Stormo G D. Pacific Symposium on Biocomputing. 1999;4:112–123. [PubMed]
5. Akutsu T, Miyano S, Kuhara S. Pacific Symposium on Biocomputing. 1999;4:17–28. [PubMed]
6. Akutsu T, Miyano S, Kuhara S. Pacific Symposium on Biocomputing. 2000;5:293–304. [PubMed]
7. Ideker T E, Thorsson V, Karp R M. Pacific Symposium on Biocomputing. 2000;5:305–316. [PubMed]
8. D'Haeseleer P, Liang S, Simogyi R. Bioinformatics. 2000;16:707–726. [PubMed]
9. Eiswirth M, Freund A, Ross J. J Phys Chem. 1991;95:1294–1299.
10. Gilman A, Ross J. Biophys J. 1995;69:1321–1333. [PMC free article] [PubMed]
11. Arkin A, Ross J. J Phys Chem. 1995;99:970–979.
12. Arkin A, Shen P, Ross J. Science. 1997;277:1275–1279.
13. Ross J, Vlad M. Annu Rev Phys Chem. 1999;50:51–78. [PubMed]
14. Vlad M O, Moran M, Ross J. Physica A. 2000;278:504–525.
15. Tsuchiya T, Ross J. J Phys Chem A. 2001;105:4052–4058.
16. Irvine D H, Savageau M A. SIAM J Num Anal. 1990;27:704–735.
17. Termonia Y, Ross J. Proc Natl Acad Sci USA. 1981;78:2952–2956. [PMC free article] [PubMed]

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