Eyring equation

The Eyring equation (occasionally also known as Eyring–Polanyi equation) is an equation used in chemical kinetics to describe changes in the rate of a chemical reaction against temperature. It was developed almost simultaneously in 1935 by Henry Eyring, Meredith Gwynne Evans and Michael Polanyi. The equation follows from the transition state theory, also known as activated-complex theory. If one assumes a constant enthalpy of activation and constant entropy of activation, the Eyring equation is similar to the empirical Arrhenius equation, despite the Arrhenius equation being empirical and the Eyring equation based on statistical mechanical justification.

General form edit

The general form of the Eyring–Polanyi equation somewhat resembles the Arrhenius equation:

\ k={\frac {\kappa k_{\mathrm {B} }T}{h}}e^{-{\frac {\Delta G^{\ddagger }}{RT}}}

where

k

is the rate constant,

\Delta G^{\ddagger }

is the Gibbs energy of activation,

\kappa

is the transmission coefficient,

k_{\mathrm {B} }

is the Boltzmann constant,

T

is the temperature, and

h

is the Planck constant.

The transmission coefficient $\kappa$ is often assumed to be equal to one as it reflects what fraction of the flux through the transition state proceeds to the product without recrossing the transition state. So, a transmission coefficient equal to one means that the fundamental no-recrossing assumption of transition state theory holds perfectly. However, $\kappa$ is typically not one because (i) the reaction coordinate chosen for the process at hand is usually not perfect and (ii) many barrier-crossing processes are somewhat or even strongly diffusive in nature. For example, the transmission coefficient of methane hopping in a gas hydrate from one site to an adjacent empty site is between 0.25 and 0.5.^[1] Typically, reactive flux correlation function (RFCF) simulations are performed in order to explicitly calculate $\kappa$ from the resulting plateau in the RFCF. This approach is also referred to as the Bennett-Chandler approach, which yields a dynamical correction to the standard transition state theory-based rate constant.

It can be rewritten as:^[2]

k={\frac {\kappa k_{\mathrm {B} }T}{h}}e^{\frac {\Delta S^{\ddagger }}{R}}e^{-{\frac {\Delta H^{\ddagger }}{RT}}}

One can put this equation in the following form:

\ln {\frac {k}{T}}={\frac {-\Delta H^{\ddagger }}{R}}\cdot {\frac {1}{T}}+\ln {\frac {\kappa k_{\mathrm {B} }}{h}}+{\frac {\Delta S^{\ddagger }}{R}}

where:

$k$ = reaction rate constant
$T$ = absolute temperature
$\Delta H^{\ddagger }$ = enthalpy of activation
$R$ = gas constant
$\kappa$ = transmission coefficient
$k_{\mathrm {B} }$ = Boltzmann constant = R/N_A, N_A = Avogadro constant
$h$ = Planck constant
$\Delta S^{\ddagger }$ = entropy of activation

If one assumes constant enthalpy of activation, constant entropy of activation, and constant transmission coefficient, this equation can be used as follows: A certain chemical reaction is performed at different temperatures and the reaction rate is determined. The plot of $\ln(k/T)$ versus $1/T$ gives a straight line with slope $-\Delta H^{\ddagger }/R$ from which the enthalpy of activation can be derived and with intercept $\ln(\kappa k_{\mathrm {B} }/h)+\Delta S^{\ddagger }/R$ from which the entropy of activation is derived.

Accuracy edit

Transition state theory requires a value of the transmission coefficient, called $\kappa$ in that theory. This value is often taken to be unity (i.e., the species passing through the transition state $AB^{\ddagger }$ always proceed directly to products $AB$ and never revert to reactants $A$ and $B$ ). To avoid specifying a value of $\kappa$ , the rate constant can be compared to the value of the rate constant at some fixed reference temperature (i.e., $\ k(T)/k(T_{\rm {Ref}})$ ) which eliminates the $\kappa$ factor in the resulting expression if one assumes that the transmission coefficient is independent of temperature.

Error propagation formulas edit

Error propagation formulas for $\Delta H^{\ddagger }$ and $\Delta S^{\ddagger }$ have been published.^[3]

Notes edit

^ Peters, B.; Zimmermann, N. E. R.; Beckham, G. T.; Tester, J. W.; Trout, B. L. (2008). "Path Sampling Calculation of Methane Diffusivity in Natural Gas Hydrates from a Water-Vacancy Assisted Mechanism". J. Am. Chem. Soc. 130 (51): 17342–17350. doi:10.1021/ja802014m. hdl:11420/6551. PMID 19053189.
^ Espenson, James H. (1981). Chemical Kinetics and Reaction Mechanisms. McGraw-Hill. p. 117. ISBN 0-07-019667-2.
^ Morse, Paige M.; Spencer, Michael D.; Wilson, Scott R.; Girolami, Gregory S. (1994). "A Static Agostic α-CH-M Interaction Observable by NMR Spectroscopy: Synthesis of the Chromium(II) Alkyl [Cr₂(CH₂SiMe₃)₆]^2- and Its Conversion to the Unusual "Windowpane" Bis(metallacycle) Complex [Cr(κ²C,C-CH₂SiMe₂CH₂)₂]^2-". Organometallics. 13: 1646. doi:10.1021/om00017a023.

References edit

Evans, M.G.; Polanyi M. (1935). "Some applications of the transition state method to the calculation of reaction velocities, especially in solution". Trans. Faraday Soc. 31: 875–894. doi:10.1039/tf9353100875.
Eyring, H. (1935). "The Activated Complex in Chemical Reactions". J. Chem. Phys. 3 (2): 107–115. Bibcode:1935JChPh...3..107E. doi:10.1063/1.1749604.
Eyring, H.; Polanyi, M. (2013-11-01). "On Simple Gas Reactions". Zeitschrift für Physikalische Chemie. 227 (11): 1221–1246. doi:10.1524/zpch.2013.9023. ISSN 2196-7156. S2CID 119992451.
Laidler, K.J.; King M.C. (1983). "The development of Transition-State Theory". J. Phys. Chem. 87 (15): 2657–2664. doi:10.1021/j100238a002.
Polanyi, J.C. (1987). "Some concepts in reaction dynamics". Science. 236 (4802): 680–690. Bibcode:1987Sci...236..680P. doi:10.1126/science.236.4802.680. PMID 17748308. S2CID 19914017.
Chapman, S. and Cowling, T.G. (1991). "The Mathematical Theory of Non-uniform Gases: An Account of the Kinetic Theory of Viscosity, Thermal Conduction and Diffusion in Gases" (3rd Edition). Cambridge University Press, ISBN 9780521408448

External links edit

[PetersJACS2008-1] Peters, B.; Zimmermann, N. E. R.; Beckham, G. T.; Tester, J. W.; Trout, B. L. (2008). "Path Sampling Calculation of Methane Diffusivity in Natural Gas Hydrates from a Water-Vacancy Assisted Mechanism". J. Am. Chem. Soc. 130 (51): 17342–17350. doi:10.1021/ja802014m. hdl:11420/6551. PMID 19053189.

[2] Espenson, James H. (1981). Chemical Kinetics and Reaction Mechanisms. McGraw-Hill. p. 117. ISBN 0-07-019667-2.

[3] Morse, Paige M.; Spencer, Michael D.; Wilson, Scott R.; Girolami, Gregory S. (1994). "A Static Agostic α-CH-M Interaction Observable by NMR Spectroscopy: Synthesis of the Chromium(II) Alkyl [Cr₂(CH₂SiMe₃)₆]^2- and Its Conversion to the Unusual "Windowpane" Bis(metallacycle) Complex [Cr(κ²C,C-CH₂SiMe₂CH₂)₂]^2-". Organometallics. 13: 1646. doi:10.1021/om00017a023.

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