5.4: The Kinetics of Enzymatic Catalysis
- Page ID
- 234008
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Michaelis-Menten Enzyme Kinetics
Enzymes are highly specific catalysts for biochemical reactions, with each enzyme showing a selectivity for a single reactant, or substrate. Many enzyme–substrate reactions follow a simple mechanism that consists of the initial formation of an enzyme–substrate complex, \(ES\), which subsequently decomposes to form product, releasing the enzyme to react again.
This is described within the following multi-step mechanism for a reversible reaction catalyzed by an enzyme
\[ E + S \underset{k_{-1}}{\overset{k_1}{\rightleftharpoons}} ES \underset{k_{-2}}{\overset{k_2}{\rightleftharpoons}} E + P \label{13.20}\]
where \(k_1\), \(k_{–1}\), \(k_2\), and \(k_{–2}\) are rate constants for the forward and backward reactions. The reaction’s rate law for generating the product \([P]\) is
\[ reaction rate = \dfrac{d[P]}{dt} = k_2[ES] - k_{-2}[E][P] \label{13.21A}\]
However, if we make measurement early in the reaction, the concentration of products is negligible, i.e.,
\[[P] \approx 0\]
and we can ignore the back reaction (second term in right side of Equation \(\ref{13.21A}\)). Then under these conditions, the reaction’s rate is
\[ reaction rate = \dfrac{d[P]}{dt} = k_2[ES] \label{13.21}\]
To be analytically useful we need to write Equation \(\ref{13.21}\) in terms of the reactants, e.g., the concentrations of enzyme and substrate, which are the independent variables we can control when setting up an experiment. To do this we use the steady-state approximation, in which we assume that the concentration of \(ES\) remains essentially constant. Following an initial period, during which the enzyme–substrate complex first forms, the rate at which \(ES\) forms
\[ \dfrac{d[ES]}{dt} =k_1[E] [S] = k_1([E]_0 − [ES])[S] \label{13.22}\]
is equal to the rate at which it disappears
\[ − \dfrac{d[ES]}{dt} = k_{−1}[ES] + k_2[ES] \label{13.23}\]
where \([E]_0\) is the enzyme’s original concentration. Combining Equations \(\ref{13.22}\) and \(\ref{13.23}\) gives
\[k_1([E]_0 − [ES]) [S] = k_{−1}[ES] + k_2[ES]\]
which we solve for the concentration of the enzyme–substrate complex
\[ [ES] = \dfrac{ [E]_0[S] }{ \dfrac{k_{−1} + k_2}{k_1} + [S] } = \dfrac{[E]_0[S] }{K_m + [S]} \label{Eq13.24}\]
where \(K_m\) is the Michaelis constant. Substituting Equation \(\ref{Eq13.24}\) into Equation \(\ref{13.21}\) leaves us with the rate equation.
\[ \dfrac{d[P]}{dt} = reaction rate = \dfrac{k_2[E]_0[S]}{K_m + [S]} \label{Eq13.25}\]
The factor k_{2}[E]_{0} equals the maximum possible rate at a given initial concentration of enzyme, that is k_{2}[E]_{0} = V_{max}. Therefore Equation \(\ref{Eq13.25}\) simplifies to
\[ \dfrac{d[P]}{dt} = reaction rate = \dfrac{V_{max}[S]}{K_m + [S]} \label{Eq13.26}\]
Equation \(\ref{Eq13.26}\) is known as Michaelis-Menten equation, and it represents how the reaction rate depends on the concentration of substrate, under normal conditions in which the concentration of substrate is always much higher than the concentration of enzyme (the catalyst). A plot of Equation \(\ref{Eq13.26}\) is shown in Figure \(\PageIndex{1}\)
From the plot, we can see that The Michaelis constant \(K_m\) is the substrate concentration at which the reaction rate is at half-maximum, and is an inverse measure of the substrate's affinity for the enzyme—as a small \(K_m\) indicates high affinity, meaning that the rate will approach \(V_{max}\) more quickly.
At lower substrate concentrations, where \([S] \ll K_m\), Equation \(\ref{Eq13.26}\) becomes
\[ \dfrac{d[P]}{dt} = \dfrac{V_{max}[S]}{K_m + [S]} \approx \dfrac{V_{max}[S]}{K_m} \label{13.27}\]
so the reaction rate increases linearly when increasing the concentration of substrate.
For high substrate concentrations, where \([S] \gg K_m\), Equation \(\ref{Eq13.26}\) simplifies to
\[ \dfrac{d[P]}{dt} = \dfrac{V_{max}[S]}{ K_m + [S]} \approx \ V_{max} \label{Eq13.27}\]
so under these conditions the reaction rate is independent of the concentration of substrate, and equals the \(V_{max}\). This is because all the enzyme is forming an ES complex and there is no free enzyme to bind to the free substrate. Therefore each cycle of catalysis must conclude before there is free enzyme to catalyze the conversation of more free substrate (the enzyme is saturated with the substrate when the concentration of substrate is too high) (see figure below)
Figure\(\PageIndex{2}\)when the substrate concentration is too high, the available enzyme binding sites become completely filled. The enzyme is saturated with substrate and the reaction rate ceases to increase beyond {V_{max} Image by GYassineMrabetTalk✉ This W3C-unspecified vector image was created with Inkscape ., Public domain, via Wikimedia Commons
Turnover number
From the last two terms in Equation \(\ref{13.27}\), we can express \(V_{max}\) in terms of a turnover number (\(k_{cat}\)):
\[ V_{max} = k_{cat}[E]_o\]
where \([E]_0\) is the enzyme concentration and \(k_{cat}\) is the turnover number, defined as the maximum number of substrate molecules converted to product per enzyme molecule per second. Hence, the turnover number is defined as the maximum number of chemical conversions of substrate molecules per second that a single catalytic site will execute for a given enzyme concentration \([E]_o\).
Example \(\PageIndex{1}\): Turnover number of acetylcholinesterase
Acetylcholinesterase (AChE) may be one of the fastest enzymes. It hydrolyzes acetylcholine to choline and an acetate group. One of the earliest values of the turnover number was \(3 \times 10^7\) (molecules of acetylcholine) per minute per molecule of enzyme. A more recent value at 25°C, pH = 7.0, acetylcholine concentration of \(2.5 \times 10^{−3}\; M\), was found to be \(7.4 \times 10^5\; min^{−1}\) (J Biol Chem. 236 (8): 2292–5.).
There may be some 30 active centers per molecule. AChE is a serine hydrolase that reacts with acetylcholine at close to the diffusion-controlled rate. A diffusion-controlled reaction occurs so quickly that the reaction rate is the rate of transport of the reactants through the solution; as quickly as the reactants encounter each other, they react.
The Significance of \(K_M\) and \(V_{max}\)
The Michaelis-Menten model is used in a variety of biochemical situations other than enzyme-substrate interaction, including antigen-antibody binding, DNA-DNA hybridization, and protein-protein interaction. It can be used to characterize a generic biochemical reaction. The experimentally determined parameters values vary wildly between enzymes (Table \(\PageIndex{1}\)):
Enzyme | \(K_m\) (M) | \(k_{cat}\) (1/s) | \(k_{cat}/K_m\) (1/M.s) |
---|---|---|---|
Chymotrypsin | 1.5 × 10^{−2} | 0.14 | 9.3 |
Pepsin | 3.0 × 10^{−4} | 0.50 | 1.7 × 10^{3} |
Tyrosyl-tRNA synthetase | 9.0 × 10^{−4} | 7.6 | 8.4 × 10^{3} |
Ribonuclease | 7.9 × 10^{−3} | 7.9 × 10^{2} | 1.0 × 10^{5} |
Carbonic anhydrase | 2.6 × 10^{−2} | 4.0 × 10^{5} | 1.5 × 10^{7} |
Fumarase | 5.0 × 10^{−6} | 8.0 × 10^{2} | 1.6 × 10^{8} |
While \(K_m\) is equal to the substrate concentration at which the enzyme converts substrates into products at half its maximal rate and hence is related to the affinity of the substrate for the enzyme. The catalytic rate \(k_{cat}\) is the rate of product formation when the enzyme is saturated with substrate and therefore reflects the enzyme's maximum rate. The rate of product formation is dependent on both how well the enzyme binds substrate and how fast the enzyme converts substrate into product once substrate is bound. For a kinetically perfect enzyme, every encounter between enzyme and substrate leads to product and hence the reaction velocity is only limited by the rate the enzyme encounters substrate in solution. From Equation \(\ref{Eq13.24}\), the catalytic efficiency of a protein can be evaluated.
\[ \dfrac{k_{cat}}{K_m} = \dfrac{k_2}{K_m} = \dfrac{k_1k_2}{k_{-1} + k_2}\]
This \(k_{cat}/K_m\) ratio is called the specificity constant measure of how efficiently an enzyme converts a substrate into product. It has a theoretical upper limit of 10^{8} – 10^{10} /M.s; enzymes working close to this, such as fumarase, are termed superefficient (Table \(\PageIndex{1}\)).
Determining \(V_m\) and \(K_m\) from experimental data can be difficult and the most common way is to determine initial rates, \(v_0\), from experimental values of \([P]\) or \([S]\) as a function of time. Hyperbolic graphs of \(v_0\) vs. \([S]\) can be fit or transformed as we explored with the different mathematical transformations of the hyperbolic binding equation to determine \(K_d\). These included:
- nonlinear hyperbolic fit (e.g., Figure \(\PageIndex{1}\))
- double reciprocal plot (e.g., Lineweaver–Burk plot discussed below
Lineweaver–Burk plot
Another commonly-used plot in examining enzyme kinetics is the Lineweaver-Burk plot, in with the inverse of the reaction rate, \(1/r\), is plotted against the inverse of the substrate concentration \(1/\left[ \text{S} \right]\). Rearranging Equation \(\ref{Eq13.26}\),
\[\dfrac{1}{r} = \dfrac{K_M + \left[ \text{S} \right]}{k_2 \left[ \text{E} \right]_0 \left[ \text{S} \right]} = \dfrac{K_M}{k_2 \left[ \text{E} \right]_0} \dfrac{1}{\left[ \text{S} \right]} + \dfrac{1}{k_2 \left[ \text{E} \right]_0} \label{Eq28}\]
The Lineweaver–Burk plot (or double reciprocal plot) is a graphical representation of the Lineweaver–Burk equation of enzyme kinetics, described by Hans Lineweaver and Dean Burk in 1934 (Figure \(\PageIndex{2}\)). The Lineweaver-Burk plot results in a straight line with the slope equal to \(K_M/k_2 \left[ \text{E} \right]_0\) and \(y\)-intercept equal to \(1/k_2 \left[ \text{E} \right]_0\) which is \(1/V_{max}\) via Equation \(\ref{Eq13.26}\).
The plot provides a useful graphical method for analysis of the Michaelis–Menten equation:
\[V = \dfrac{V_{\max} [S]}{K_m + [S]}\]
Taking the reciprocal gives
\[\dfrac{1}{V} = \dfrac {K_m + [S]} {V_{max}[S]} = \dfrac{K_m}{V_{max}} \dfrac{1}{[S]} + \dfrac{1}{V_{max}}\]
where
- \(V\) is the reaction velocity (the reaction rate),
- \(K_m\) is the Michaelis–Menten constant,
- \(V_{max}\) is the maximum reaction velocity, and
- \([S]\) is the substrate concentration.
The Lineweaver–Burk plot was widely used to determine important terms in enzyme kinetics, such as \(K_m\) and \(V_{max}\), before the wide availability of powerful computers and non-linear regression software. The y-intercept of such a graph is equivalent to the inverse of \(V_{max}\); the x-intercept of the graph represents \(−1/K_m\). It also gives a quick, visual impression of the different forms of enzyme inhibition.
Example \(\PageIndex{2}\)
The reaction between nicotineamide mononucleotide and ATP to form nicotineamide–adenine dinucleotide and pyrophosphate is catalyzed by the enzyme nicotinamide mononucleotide adenylyltransferase. The following table provides typical data obtained at a pH of 4.95. The substrate, S, is nicotinamide mononucleotide and the initial rate, v, is the μmol of nicotinamide–adenine dinucleotide formed in a 3-min reaction period.
[S] (mM) | v (μmol) | [S] (mM) | v (μmol) |
---|---|---|---|
0.138 | 0.148 | 0.560 | 0.324 |
0.220 | 0.171 | 0.766 | 0.390 |
0.291 | 0.234 | 1.460 | 0.493 |
Determine values for V_{max} and K_{m}.
Solution
Figure 13.12 shows the Lineweaver–Burk plot for this data and the resulting regression equation. Using the y-intercept, we calculate V_{max} as
V_{max}= 1 / y−intercept = 1 / 1.708 mol = 0.585 mol
and using the slope we find that K_{m} is
K_{m} = slope × V_{max} = 0.7528 molimM × 0.585 mol = 0.440 mM
-diphenyl oxidase
The following data are for the oxidation of catechol (the substrate) to o-quinone by the enzyme o-diphenyl oxidase. The reaction is followed by monitoring the change in absorbance at 540 nm. The data in this exercise are adapted from jkimball.
[catechol] (mM) |
0.3 |
0.6 |
1.2 |
4.8 |
---|---|---|---|---|
rate (∆AU/min) |
0.020 |
0.035 |
0.048 |
0.056 |
Determine values for V_{max} and K_{m}.
Problems with the Method
The Lineweaver–Burk plot is classically used in older texts, but is prone to error, as the y-axis takes the reciprocal of the rate of reaction – in turn increasing any small errors in measurement. Also, most points on the plot are found far to the right of the y-axis (due to limiting solubility not allowing for large values of \([S]\) and hence no small values for \(1/[S]\)), calling for a large extrapolation back to obtain x- and y-intercepts^{.}
When used for determining the type of enzyme inhibition, the Lineweaver–Burk plot can distinguish competitive and non-competitive. Competitive inhibitors have the same y-intercept as uninhibited enzyme (since \(V_{max}\) is unaffected by competitive inhibitors the inverse of \(V_{max}\) also doesn't change) but there are different slopes and x-intercepts between the two data sets. Non-competitive inhibition produces plots with the same x-intercept as uninhibited enzyme (\(K_m\) is unaffected) but different slopes and y-intercepts.
Contributors and Attributions
David Harvey (DePauw University)
- World Public Library
- Wikipedia
- Dr. S.K. Khare (IIT Delhi) via NPTEL
- Wikipedia contributors. (2021, May 14). Enzyme kinetics. In Wikipedia, The Free Encyclopedia. Retrieved 17:48, May 17, 2021, from https://en.wikipedia.org/w/index.php?title=Enzyme_kinetics&oldid=1023054417