Kinetic Theory and Reaction Kinetics - Bioprocess Engineering: Kinetics, Biosystems, Sustainability and Reactor Design - page 257

CHAPTER
6

Kinetic Th eory and Reactio n Kinetics

OUTLINE

6.1. Elementary Kinetic Theory 258 6.3.2. Pseudosteady-State Hypothesis 269

6.1.1. Distribution Laws 258

6.4. Unimolecular Reactions 270

6.1.2. Collision Rate 263

6.5. Free Radicals 272

6.2. Collision Theory of Reaction Rates 264

6.6. Kinetics of Acid Hydrolysis 274

6.3. Reaction Rate Analysis/
Approximation

267 6.7. Summary 277

6.3.1. Fast-Equilibrium Step
Approximation

Problems 278

268

We learned that the reaction rate plays a key role in bioprocess analysis. The reaction rate is
the main interest of bioprocess kinetics. In Chapter 3, we learned that the rate of reaction is
observed as functions of temperature and concentrations. Based on equilibrium analysis, we
further showed that the reaction rate variation with temperature is due to the reaction energy
requirement. We also learned that the most commonly used experimental reaction rate law
form is power-law form in concentrations. In particular, when nonequilibrium arguments
were applied to an elementary reaction,
X

N S

n j A j ¼ 0 (6.1)

j ¼1

The rate of reaction may be written as Eqn (3.52) or

k ðe DG f =RT e DG b =RT

r ¼ Þ (6.2)

If the heat capacity is independent on temperature and activity coefficients are independent
on the concentrations, the rate expression can be reduced to Eqn (3.101) or