Abstract
Reaction kinetics deals with the question how fast a chemical reaction proceeds. From a mathematical point of view, problems in reaction kinetics are formulated as rate equations, i.e., differential equations in time. In the limit t → ∞ the results of reaction kinetics and thermodynamics (chemical equilibrium) must coincide. We consider this in detail in Problem 6.4. At the end of the chapter we deal with the fascinating field of autocatalysis and oscillating chemical reactions.
This is a preview of subscription content, log in via an institution to check access.
Access this chapter
Tax calculation will be finalised at checkout
Purchases are for personal use only
Notes
- 1.
Note that there are cases where the most general form r = k f([J 1], [J 2], …) is more appropriate.
- 2.
According to kinetic theory (Eq. (7.3)), the collision rate between N A particles of a species A and N B particles of species B at temperature T is \(N_{\text{A}}N_{\text{B}}\sigma _{\text{AB}}\left (\frac{8k_{B}T} {\mu } \right )^{\frac{1} {2} }\) where σ AB is the collision cross section and μ is the effective mass.
- 3.
See Problem 10.1.
- 4.
According to Eq. (6.19), the extent of reaction at time t 50 is \(\xi _{50} = \frac{1} {2}[\text{OH}]^{0}\).
- 5.
LASER is the abbreviation for light amplification by stimulated emission of radiation.
Reference
Lavabre D, Pemienta V, Levy G, Micheau JC (1993) J Phys Chem 97:5321
Author information
Authors and Affiliations
Rights and permissions
Copyright information
© 2017 Springer International Publishing AG
About this chapter
Cite this chapter
Vogt, J. (2017). Chemical Kinetics. In: Exam Survival Guide: Physical Chemistry. Springer, Cham. https://doi.org/10.1007/978-3-319-49810-2_6
Download citation
DOI: https://doi.org/10.1007/978-3-319-49810-2_6
Published:
Publisher Name: Springer, Cham
Print ISBN: 978-3-319-49808-9
Online ISBN: 978-3-319-49810-2
eBook Packages: Chemistry and Materials ScienceChemistry and Material Science (R0)