'Rate laws' presentation slideshows

Basics of biochemical systems theory

Basics of biochemical systems theory. I. Graphical representation of biochemical networks. Mass transport. Glucose out. Glucose in. Glucose 6-P. Fructose 6-P. Chemical conversion. Glucose. Glucose 6-P. ATP. ADP. Material flow. Glucose. Glucose 6-P. ATP. ADP. Information flow.

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Chemical Kinetics Chapter 15

Chemical Kinetics Chapter 15. An automotive catalytic muffler. Chemical Kinetics Chapter 15. We can use thermodynamics to tell if a reaction is product or reactant favored. But this gives us no info on HOW FAST reaction goes from reactants to products.

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SAMPLE EXERCISE 14.1 Calculating an Average Rate of Reaction

SAMPLE EXERCISE 14.1 Calculating an Average Rate of Reaction. From the data given in the caption of Figure 14.3 , calculate the average rate at which A disappears over the time interval from 20 s to 40 s. Solution

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Chemical Equilibrium

Chemical Equilibrium. Brown, LeMay Ch 15 AP Chemistry Monta Vista High School. 15.1: Chemical Equilibrium. Occurs when opposing reactions are proceeding at the same rate Forward rate = reverse rate of reaction Ex: Vapor pressure: rate of vaporization = rate of condensation

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Chemical Reaction Engineering Asynchronous Video Series

Chemical Reaction Engineering Asynchronous Video Series. Chapter 4, Part 1: Applying the Algorithm to a CSTR H. Scott Fogler, Ph.D. Summary. At the start of the chapter we saw we needed -r A =f(X). This result is achieved in two steps. Rate Laws -r A =k f(C i )

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Lecture 5

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Lecture 5

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Development of Reliable, Simple Rate Expressions from a Microkinetic Model of FTS on Cobalt

Development of Reliable, Simple Rate Expressions from a Microkinetic Model of FTS on Cobalt. Calvin H. Bartholomew, George Huber, and Hu Zou Brigham Young University And George Huber, Rahul Nabar, Peter Ferrin, Manos Mavrikakis, and James Dumesic University of Wisconsin, Madison.

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Lecture 5 Thursday 1/17/08

Lecture 5 Thursday 1/17/08. Block 1: Mole Balances Block 2: Rate Laws Block 3: Stoichiometry Stoichiometric Table: Flow Definitions of Concentration: Flow Gas Phase Volumetric Flow rate Calculate the Equilibirum Conversion X e.

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Zero and First-Order Rate Reactions

Zero and First-Order Rate Reactions. Samir Kumar Khanal, Ph.D. Department of Civil, Construction and Environmental Engineering Iowa State University. Question!! Assume you are a process engineer (biological), newly recruited by P & G. In your first week of job, you have been assigned

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Chapter 15

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Lecture 14

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Rates and Rate Laws

Rates and Rate Laws. Reaction Rate. The change in concentration of a reactant or product per unit of time. Reaction Rates:. 2NO 2 (g) ? 2NO(g) + O 2 (g). 1. Can measure disappearance of reactants. 2. Can measure appearance of products. 3. Are proportional

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Chapter 14: Rates of Reaction

Chapter 14: Rates of Reaction. Chemistry 1062: Principles of Chemistry II Andy Aspaas, Instructor. Chemical kinetics. Study of the rate or speed of reactions Rate may be affected by any of the following: Concentration of reactants Presence or concentration of a catalyst

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Chemistry 1011

Chemistry 1011. TOPIC Rate of Reaction TEXT REFERENCE Masterton and Hurley Chapter 11. 11.7 Reaction Mechanisms. YOU ARE EXPECTED TO BE ABLE TO: Define reaction mechanism and show how the reaction order is dependent upon the mechanism by which a reaction takes place.

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Lecture 7

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Chemical Reaction Engineering Asynchronous Video Series

Chemical Reaction Engineering Asynchronous Video Series. Chapter 4, Part 4: Membrane Reactors H. Scott Fogler, Ph.D. Membrane Reactors. Membrane Reactors. For membrane reactors, we cannot use conversion. We have to work in terms of the molar flow rates F A , F B , F C. Membrane Reactors.

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Types of Rate Laws

Types of Rate Laws. Differential Rate Laws i.e. The rate law or rate equations Rate is given as a function of concentration of reactants Takes the form for A + B --> C rate = k[A] a [B] b use inital rate data to determine order with respect to each reactant rate constant.

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Kinetics

Kinetics. Brainstorm: What are some factors that affect the rate of a reaction?. Reaction Rate. Change in [reactants] or [products] per unit time (M/s) Always expressed as a positive quantity Can be expressed as appearance of B OR disappearance of A. A ? B. Changes in reaction rate.

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