# 6.6: Enzyme Kinetics as an Approach to Understanding Mechanism

- Page ID
- 14950

## Rapid Equilibrium Enzyme-Catalyzed Reactions

We have previously derived equations for the reversible binding of a ligand to a macromolecule. Next we derived equations for the receptor-mediated facilitated transport of a molecule through a semipermeable membrane. This latter case extended the former case by the addition of a physical transport step. Now, in what hopefully will seem like dï¿½jï¿½ vu, we will derive almost identical equations for the chemical transformation of a ligand, commonly referred to as a substrate, by an enzyme. Two scenarios will be studied.

- Rapid Equilibrium Assumption - enzyme E (macromolecule) and substrate S (ligand) concentrations can be determined using the dissociation constant since E, S, and ES are in rapid equilibrium, as we previously used in our derivation of the equations for facilitated transport. Sorry about the switch from A to S in designation of substrate. Biochemists use S to represent the substrate (ligand) but also use A, B, and P and Q to represent reactant and products in the case of multi-substrate and multi-product reactions.
- Steady State Assumption (more general) - enzyme and substrate concentrations are not those determined using the dissociation constant.

Enzyme kinetics experiments, as we will see in the next several chapters, must be used to determine the detailed mechanism of the catalyzed reaction. Using kinetics analyzes you can determine the order of binding/dissociation of substrates and products, the rate constants for individual steps, and clues as the to methods used by the enzyme in catalysis.

Consider the following reaction mechanism for the enzyme-catalyzed conversion of substrate S into product P. (We will assume that the catalyzed rate is much greater than the noncatalyzed rate.)

As we did for the derivation of the equations for the facilitated transport reactions under rapid equilibrium conditions, this derivation is based on the assumption that the relative concentrations of S, E, and ES can be determined by the dissociation constant, Ks, for the interactions and the concentrations of each species during the early part of the reaction (i.e. under initial rate conditions). Assume also the S >> Eo. Remember that under these conditions, S does not change much with time. Is this a valid assumption? Examine the mechanism shown above. S binds to E with a second order rate constant k1. ES has two fates. It can dissociate with a first order rate constant k2 to S + E, or it can be converted to product with a first order rate constant of k3 to give P + E. If we assume that k2 >> k3 (i.e. that the complex falls apart much more quickly than S is converted to P), then the relative ratios of S, E, and ES can be described by Ks. Alternatively, you can think about it this way. If S binds to E, most of S will dissociate, and a small amount will be converted to P. If it does, then E is now free, and will quickly bind S and reequilibrate since the most likely fate of bound S is to dissociate, not be converted to P (since k3 << k2). This make sense also, if you consider that the physical step characterized by k2 is likely to be quicker than the chemical step, characterized by k3. Hence the following assumptions have been used:

- S >> Eo
- Po = 0
- k3 is rate limiting (i.e. the slow step)

We would like to derive equations which show the velocity v as a function of the initial substrate concentration, So , (assuming that P is negligible over the time course of measuring the initial velocity). Also assume that the v catalyzed >> vnoncatalyzed. In contrast to the first-order reaction of S to P in the absence of E, v is not proportional to So but rather to Sbound. as we described in class with facilitated diffusion (flux proportional to AR, not free A). Therefore,

v **α** ES, or

Equation 1) v = const [ES] = k3 [ES]

where v is the velocity. How can we calculate ES when we know S (which is equal to So) and Etot (which is Eo)? Let us assume that S is much greater than E, as is the likely biological case. We can calculate ES using the following equations and the same procedure we used for the derivation of the binding equation, which gives the equation below:

ES = (EoS)/(Ks + S) (analogous to ML = (MoL)/(Kd + L)

DERIVATION

Equation 5) v = const [ES] = k3 [ES] = k3 EoS/(Ks + S) = VmS/(Ks + S).

This is the world famous Henri-Michaelis-Menten Equation

Just as in the case with noncatalyzed first order decay, it is easiest to measure the initial velocity of the reaction when [S] does not change much with time and the velocity is constant (i.e the slope of the dP/dt curve is constant). A plot of [P] vs t (called a progress curve) is made for each different substrate concentration studied. From these curves, the initial rates at each [S] is determined. Alternatively, one set reaction time is determined for all the different substrates concentrations that gives a linear rise in [P] with time. At the time, the reaction can be stopped (quenched) with a reagent that does not cause any change in S or P. Initial rates can be easily calculated for each [S] from a single data point in this case. i

- a plot of v vs S is hyperbolic
- v = 0 when S = 0
- v is a linear function of S when S<<Ks.
- v = Vmax (or Vm) when S is much greater than Ks
- S = Ks when v = Vmax/2.

These are the same conditions we detailed for our understanding of the binding equation

ML = (MoL)/(Kd + L)

The interactive Mathematics graph below allows you to change the relative value of Vm and Ks (which in the graph is given the more general name of Km). Note that when Km is not << S, the graph does not reach saturation and does not look hyperbolic. It should be apparent from the graph that only if S >> Km (or when S is approximately 100x greater than Km) will saturation be achieved.

Wolfram Mathematica CDF Player - Michaelis-Menten Equation (free plugin required)

Interactive SageMath Graph: Michaelis-Menten Equation

Very often these graphs are transformed into double reciprocal or Lineweaver-Burk plots as shown below. These plots can be used to estimate Vm from the 1/v intercept (1/Vm) and Km from the 1/S axis (-1/Km). These values should be used as "seed" values for a nonlinear fit to the hyperbola that models the actual v vs D curve.

Wolfram Mathematica CDF Player - Lineweaver-Burk Plot: 1/v vs 1/[S](free plugin required)

Interactive SageMath Graph: Lineweaver Burk Plot

- History and Picture of Maude Menten

As we saw in the graph of A or P vs t for a noncatalyzed, first order reaction, the velocity of the reaction, given as the slope of those curves, is always changing. Which velocity should we use in Equation 5? The answer invariably is the initial velocity measured in the early part of the reaction when little substrate is depleted. Hence v vs S curves for enzyme catalyzed reactions invariably are really v0 vs [S].

## Steady State Enzyme-Catalyzed Reactions

In this derivation, we will consider the following equations and all the rate constants, and will not arbitrarily assume that k2 >> k3. We will still assume that S >> Eo and that Po = 0. An added assumption, however, is that dES/dt is approximately 0. Look at this assumption this way. When an excess of S is added to E, ES is formed. In the rapid equilibrium assumption, we assumed that it would fall back to E + S faster than it would go onto product. In this case, we will assume that it might go on to product either less or more quickly than it will fall back to E + S. In either case, a steady state concentration of ES arises within a few milliseconds, whose concentration does not change significantly during the initial part of the reaction under which the initial rates are measured. Therefore, dES/dt is about 0. In the rapid equilibrium derivation, we observed that v = k3ES. We then solved for ES using Ks and mass balance of E. In the steady state assumption, the equation v = k3ES still holds, but know we will solve for ES using the steady state assumption that dES/dt =0.

Equation 1) v = k3ES

Equation 6: (steady state) dES/dt = k1(E)(S) - k2(ES) -k3(ES) = 0

k1(E)(S) = (k2 + k3)(ES)

k1(Eo-ES)(S) = (k2 + k3)(ES)

k1(Eo)(S) - k1(ES)(S) = (k2 + k3)(ES)

k1(Eo)(S) = (k2 + k3)(ES) + k1(ES)(S)

k1(Eo)(S) = ES (k2 + k3 + k1S)

Equation 9) v = k3ES = [k3(Eo)(S)]/ [(k2 + k3)/k1 + S] = [k3(Eo)(S)]/(Km+ S)

## Analysis of the General Michaelis-Menten Equation

This equation can be simplified and studied under different conditions. First notice that (k2 + k3)/k1 is a constant which is a function of relevant rate constants. This term is usually replaced by Km which is called the Michaelis constant (which was used in the Mathematica graph above). Likewise, when S approaches infinity (i.e. S >> Km, equation 5 becomes v = k3(Eo) which is also a constant, called Vm for maximal velocity. Substituting Vm and Km into equation 5 gives the simplified equation:

Equation 10) v = Vm(S)/(Km+ S)

It is extremely important to note that Km in the general equation does not equal the Ks, the dissociation constant used in the rapid equilibrium assumption! Km and Ks have the same units of molarity, however. A closer examination of Km shows that under the limiting case when k2 >> k3 (the rapid equilibrium assumption) then,

Equation 11) Km = (k2 + k3)/k1 = k2/k1 = Kd = Ks.

If we examine Equations 9 and 10 under several different scenarios, we can better understand the equation and the kinetic parameters:

- when S = 0, v = 0.
- when S >> Km, v = Vm = k3Eo. (i.e. v is zero order with respect to S and first order in E. Remember, k3 has units of s-1since it is a first order rate constant. k3 is often called the turnover number, because it describes how many molecules of S "turn over" to product per second.
- v = Vm/2, when S = Km.
- when S << Km, v = VmS/Km = k3EoS/Km (i.e. the reaction is bimolecular, dependent on both on S and E. k3/Km has units of M-1s-1, the same as a second order rate constant.

Notice that equations 9 and 10 are exactly analysis to the previous equations we derived:

- ML = MoL/(Kd + L) for binding of L to M
- Jo = JmA/(Kd + A) for rapid equilibrium binding and facilitated transport of A
- vo = VmS/(Ks + S) for rapid equilbirum binding and catalytic conversion of A to P.
- vo = Vm(S)/(Km+ S) for steady state binding and catalytic conversion of A to P.

Please notice that all these equations give hyperbolic dependencies of the y dependent variable (ML, Jo, and vo) on the ligand, solute, or substrate concentration, respectively.

## More Complicated Enzyme-catalyzed Reactions

Not all reactions can be characterized so simply as a simple substrate interacting with an enzyme to form an ES complex, which then turns over to form product. Sometimes, intermediates form. For example, a substrate S might interact with E to form a complex, which then is cleaved to products P and Q. Q is released from the enzyme, but P might stay covalently attached. This happens often in the hydrolytic cleavage of a peptide bond by a protease, when an activated nucleophile like Ser reacts with the sessile peptide bond in a nucleophilic substitution reaction, releasing the amine end of the former peptide bond as the leaving group, while the carboxy end of the peptide bond remains bonded to the Ser as an Ser-acyl intermediate. Water then enters and cleaves the acyl intermediate, freeing the carboxyl end of the original peptide bond. This is shown in the written reaction below:

To simplify the derivation of the kinetic equation, let's assume that E, S, and ES are in rapid equilibrium defined by the dissociation constant, Ks. Assume Q has a visible absorbance, so it is easy to monitor. Assume from the steady state assumption that:

d[E-P]/dt = k2[ES] - k3[E-P] = 0 (assuming k3 is a pseudo first order rate constant and [H2O] doesn't change.

The velocity depends on which step is rate limiting. If k3<<k2, then the k3 step is rate-limiting. Then

v = k3[E-P]

If k2<<k3, then the k2 step is rate-limiting. Then

v = k2[ES]

For a homework assignment, you derived the following kinetic equation for this reaction, assuming v = k2[ES].

You can verify that you get the same equation if you assume that v = k3[E-P]. (Also, kcat will be defined below.)

This equation looks quite complicated, especially if you substitute for Ks, k-1/k1. All the kinetic constants can be expressed as functions of the individual rate constants. However this equation can be simplified by realizing the following:

- When S >> [Ks(k3)/(k2+k3)], v = [(k2k3)/(k2 + k3)]Eo = Vm
- [Ks(k3)/(k2+k3)] = constant = Km

Substituting these into equation 7 gives:

Equation 13) v = Vm(S)/(Km+ S)

This again is the general form of the Michaelis-Menten equation

Note in the first bulleted item above that for this reaction, Vm = [(k2k3)/(k2 + k3)]Eo

This is more complicated than our earlier definition of Vm = k3Eo. They are similar in that the term Eo is multiplied by a constant which is itself a function of rate constant(s). The rate constants are generally lumped together into a generic constant called kcat. For the simple reaction **k**cat** = k3** but for the more complicated reaction with a covalent intermdiate which we just deived, **k**cat** = (k2k3)/(k2 + k3)**. For all reactions,

Equation 14) Vm = kcatEo.

Figure: Summary of vo vs S equations - Meanings of Km, kcat and Vm.

avigation

## Meaning of Kinetic Constants

It is important to get a "gut-level" understanding of the significance of the rate constants. Here they are:

- Km: The Michaelis constant with units of molarity (M), is operationally defined as the substrate concentration at which the initial velocity is half of Vmax. It is equal to the dissociation constant of E and S only in if E, S and ES are in rapid equilibrium. It can be thought of as an "effective" Kd in other cases.
- kcat: The catalytic rate constants, with units of s-1 is often called the turnover number. It is a measure of how many bound substrate molecules turnover or form product in 1 second. This is evident from equation v0 = kcat[ES]
- kcat/Km: Under condition when [S] << Km, the Michaelis-Menten equation becomes v0 = (kcat/KM)[E0][S]. This really describes a biomolecular rate constant, with units of M-1s-1, for conversion of free substrate to product. Some enzyme have kcat/Km values around 108, indicating that they are diffusion controlled. That implies that the reaction is essentially done as soon as the enzyme and substrate collide. The constant kcat/Km is also referred to as the specificity constant in that it describes how well an enzyme can differentiate between two different competing substrates. (We will show this mathematically in the next chapter.)

Table: Km and kcat values for various enzymes

Km values | ||

enzyme | substrate | Km (mM) |

catalase | H2O2 | 25 |

hexokinase (brain) | ATP | 0.4 |

D-Glucose | 0.05 | |

D-Fructose | 1.5 | |

carbonic anhydrase | HCO3- | 9 |

chymotrypsin | glycyltyrosinylglycine | 108 |

N-benzoyltyrosinamide | 2.5 | |

b-galactosidase | D-lactose | 4.0 |

threonine dehydratase | L-Thr | 5.0 |

kcat values | ||

enzyme | substrate | kcat (s-1) |

catalase | H2O2 | 40,000,000 |

carbonic anhydrase | HCO3- | 400,000 |

acetylcholinesterase | acetylcholine | 140,000 |

b-lactamase | benzylpenicillin | 2,000 |

fumarase | fumarate | 800 |

RecA protein (ATPase) | ATP | 0.4 |

Table: diffusion controlled enzymes

Enzymes with kcat/Km values close to diffusion controlled (108 - 109 M-1s-1) | ||||

enzyme | substrate | kcat (s-1) | Km (M) | kcat/Km (M-1s-1) |

acetylcholinesterase | acetylcholine | 1.4 x 104 | 9 x 10-5 | 1.6 x 108 |

carbonic anhydrase | CO2 | 1 x 106 | 1.2 x 10-2 | 8.3 x 107 |

HCO3- | 4 x 105 | 2.6 x 10-2 | 1.5 x 107 | |

catalase | H2O2 | 4 x 107 | 1.1 | 4 x 107 |

crotonase | crotonyl-CoA | 5.7 x 103 | 2 x 10-5 | 2.8 x 108 |

fumarase | fumarate | 8 x 102 | 5 x 10-6 | 1.6 x 108 |

malate | 9 x 102 | 2.5 x 10-5 | 3.6 x 107 | |

triose phosphate isomeraser | glyceraldehyde-3-P | 4.3 x 103 | 4.7 x 10-4 | 2.4 x 108 |

b-lactamase | benzylpenicillin | 2.0 x 103 | 2 x 10-4 | 1 x 108 |

Navigation

## Experimental Determination of Vmax and Km

How can Vm and Km be determined from experimental data?

a. From initial rate data: The most common way is to determine initial rates, v0, from experimental values of P or S as a function of time. Hyperbolic graphs of v0 vs [S] can be fit be fit or transformed as we explored with the different mathematical transformations of the hyperbolic binding equation to determine Kd. These included:

- nonlinear hyperbolic fit
- double reciprocal plot
- Scatchard plot

The double-reciprocal plot is commonly used to analyze initial velocity vs substrate concentration data. When used for such purposes, the graphs are referred to as Lineweaver-Burk plots, where plots of 1/v vs 1/S are straight lines with slope m = Km/Vmax, and y intercept b = 1/Vmax.

Wolfram Mathematica CDF Player - Lineweaver-Burk Plot: 1/v vs 1/[S](free plugin required)

Interactive SageMath Graph: Lineweaver Burk Plot

These plots can not be analyzed using linear regression, however, since that method assumes constant error in the y axis (in this case 1/v) data. A weighted linear regression or even better, a nonlinear fit to a hyperbolic equation should be used. The Mathcad template below shows such a nonlinear fit. A rearrangement of the corresponding Scatchard equations in the Eadie-Hofstee plot is also commonly used, especially to visualize enzyme inhibition data as we will see in the next chapter.

Mathcad 8 - Nonlinear Hyperbolic Fit. Vm and Km.

Common Error in Biochemistry Textbooks: The Shape of the Hyperbola

b. From integrated rate equations: KM and Vm can be extracted from progress curves of A or P as a function of t at one single A0 concentration by deriving an integrated rate equation for A or P as a function of t, as we did in equation 2 which shows the integrated rate equation for the conversion of A --> P in the absence of enzyme. In principle this method would be better than the initial rates methods. Why? One reason is that is not easy to be certain you are measuring the initial rate for each and every [S] which should vary over a wide range. It's also time intensive. In addition, think how much of the data is discarded if you take an entire progress curve at each substrate concentration, especially if you quench the reaction at a given time point, which effectively limits the data to one time point per substrate.

In practice, the mathematics are complicated as it is not possible to get a simple explicit function of [P] or [S] as a function of time. Nevertheless, progress has been made in progress curve analysis (no pun intended). Let us consider the simple case of a single substrate S (or A) being converted to product P in an enzyme catalyzed reaction. The analogous equations for first order, non-catalyzed rates were

A=Aoe-k1t or P = A0(1-e-k1t).

Now let's derive the equations for the enzyme-catalyzed reaction.

The derivation of the relevant equations are shown below.

A graph of P/t vs [ln (1-P/S0)]/t (shown below) from equation 18 gives a straight line with a slope of Km and a y intercept of Vm. Note that the calculated values of Vm and Km are derived from only one substrate concentration, and the values may be affected by product inhibition

Figure: Enzyme Kinetics Progress Curve

A comparison of the progress curves for the noncatalyzed 1st order reaction of S to P (red) and the enzyme catalyzed reaction (blue) is shown below. (Many thanks to Gregory Bard, UW Stout, for help with the Sage Math code). Note that the curves are similar but different. Adjust the sliders to better compare the two. If you didn't know an enzyme was present, you could easily fit the data to a first order rise in [P] with time, but it would not be the optimal fit. The progress curve in the presence of enzyme is ideal in that product inhibition is not part of the model, which would greatly complicate the analysis.

Interactive SageMath Graph: [P] vs t for enzyme catalyzed (blue) and non-enzyme catalyzed 1st order conversion, S to P

Can a simple explicit equation of P vs t be derived? The answer is no. However it can be represented by an explicit Lambert function as shown in the derivation below.

Navigation