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Lecture

Internal Mass Transfer Limitations

In course

ChE-403: Heterogeneous reaction engineering

The theoretical background and practical aspects of heterogeneous reactions including the basic knowledge of heterogeneous catalysis are introduced. The fundamentals are given to allow the design of multiphase chemical reactors. ...

Description

This lecture discusses the calculation of observed rates in the presence of internal mass transfer limitations, emphasizing the concentration in the entire pellet. Equations for steady-state processes and flux entering the pellet are analyzed for different reaction orders and particle geometries.

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Instructors (2)

Jeremy Luterbacher

Masters degree in Chemical Engineering obtained in 2007 at the Swiss Federal Institute of Technology, Lausanne (EPFL) (enrolled fall 2005, currently in 3rd semester). Relevant courses: Advanced Separation Processes, Advanced Chemical Reaction Engineering, Process Development and Polymer Chemistry and Macromolecular Engineering. - Bachelors degree in Chemistry and Chemical Engineering obtained in 2005 at the Swiss Federal Institute of Technology, Lausanne (EPFL). Relevant courses: Transport phenomena, Separation processes, Process command, Applied Energetics, Chemical Reaction Engineering, Chemical Kinetics, Quantum chemistry and Thermodynamics. - High school Maturity completed at the Nyon High School, 2002 (major subjects: biology-chemistry, advanced math, and Latin). Maturity essay completed 12-2001 with distinction - Secondary School certificate obtained in 1999 at the Gland secondary School, Latin-Greek section

Albert Renken

Official source

Related concepts (32)

Reaction rate

The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. For example, the oxidative rusting of iron under Earth's atmosphere is a slow reaction that can take many years, but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second.

Rate equation

In chemistry, the rate law or rate equation for a chemical reaction is a mathematical equation that links the rate of forward reaction with the concentrations or pressures of the reactants and constant parameters (normally rate coefficients and partial reaction orders). For many reactions, the initial rate is given by a power law such as where [\mathrm{A}] and [\mathrm{B}] express the concentration of the species \mathrm{A} and \mathrm{B}, usually in moles per liter (molarity, M).

Concentration

In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture. Several types of mathematical description can be distinguished: mass concentration, molar concentration, number concentration, and volume concentration. The concentration can refer to any kind of chemical mixture, but most frequently refers to solutes and solvents in solutions. The molar (amount) concentration has variants, such as normal concentration and osmotic concentration. Dilution is reduction of concentration, e.

Hyperbolic functions

In mathematics, hyperbolic functions are analogues of the ordinary trigonometric functions, but defined using the hyperbola rather than the circle. Just as the points (cos t, sin t) form a circle with a unit radius, the points (cosh t, sinh t) form the right half of the unit hyperbola. Also, similarly to how the derivatives of sin(t) and cos(t) are cos(t) and –sin(t) respectively, the derivatives of sinh(t) and cosh(t) are cosh(t) and +sinh(t) respectively. Hyperbolic functions occur in the calculations of angles and distances in hyperbolic geometry.

Molar concentration

Molar concentration (also called molarity, amount concentration or substance concentration) is a measure of the concentration of a chemical species, in particular of a solute in a solution, in terms of amount of substance per unit volume of solution. In chemistry, the most commonly used unit for molarity is the number of moles per liter, having the unit symbol mol/L or mol/dm3 in SI unit. A solution with a concentration of 1 mol/L is said to be 1 molar, commonly designated as 1 M.

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