This chapter discusses reaction kinetics and mechanisms. It explains that reaction mechanisms show the specific steps by which reactants are converted to products. Collision theory is used to interpret reactions, where molecules must collide with sufficient energy and proper orientation for a reaction to occur. The activation energy is the minimum energy needed to form an activated complex or transition state. Reaction mechanisms must satisfy the overall balanced chemical equation and agree with the experimentally determined rate law. Catalysts are discussed as substances that increase the rate of reactions without being consumed.
Definition of reaction kinetics, law of mass action, rates of reaction- zero, first, second, pseudo zero & pseudo first order reaction, molecularity of reaction, determination of reaction order- graphic method, substitution method, half life method.
Definition of reaction kinetics, law of mass action, rates of reaction- zero, first, second, pseudo zero & pseudo first order reaction, molecularity of reaction, determination of reaction order- graphic method, substitution method, half life method.
This is a lecture is a series on combustion chemical kinetics for engineers. The course topics are selections from thermodynamics and kinetics especially geared to the interests of engineers involved in combusition
My notes for A2 Chemistry Unit 4, typed by me and compiled from various sources. I cannot trace back where everything came from but again shall any intellectual property rights be violated, please comment /contact me and I will try my best to rectify them as soon as possible.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
Provides information about the time it takes for a chemical reaction to occur
3. Provides information about the series of elementary steps which lead to the formation of product
This slide completely describes you about the stuff include in it and also everything about chemical engineering. Fluid Mechanics. Thermodynamics. Mass Transfer Chemical Engineering. Energy Engineering, Mass Transfer 2, Heat Transfer,
This is a lecture is a series on combustion chemical kinetics for engineers. The course topics are selections from thermodynamics and kinetics especially geared to the interests of engineers involved in combusition
My notes for A2 Chemistry Unit 4, typed by me and compiled from various sources. I cannot trace back where everything came from but again shall any intellectual property rights be violated, please comment /contact me and I will try my best to rectify them as soon as possible.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
Provides information about the time it takes for a chemical reaction to occur
3. Provides information about the series of elementary steps which lead to the formation of product
This slide completely describes you about the stuff include in it and also everything about chemical engineering. Fluid Mechanics. Thermodynamics. Mass Transfer Chemical Engineering. Energy Engineering, Mass Transfer 2, Heat Transfer,
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
4. A Molecular Representation of the Elementary Steps in the Reaction of NO 2 and CO Overall: NO 2 + CO NO + CO 2 Step 1: NO 2 + NO 2 NO 3 + NO (k 1 ) Step 2: NO 3 + CO NO 2 + CO 2 (k 2 ) NO 3 is an intermediate
95. A Molecular Representation of the Elementary Steps in the Reaction of NO 2 and CO Overall: NO 2 + CO NO + CO 2 Step 1: NO 2 + NO 2 NO 3 + NO (k 1 ) Step 2: NO 3 + CO NO 2 + CO 2 (k 2 ) NO 3 is an intermediate
Fig. 12.9 Z5e 584 NO 2 + NO 2 ---> NO 3 + NO (k 1 ) NO 3 + CO ---> NO 2 + CO 2 (k 2 ) NO 3 is an intermediate Each rx called an elementary step ; I.e., its rate law can be written from its molecularity Molecularity is defined as the # of species that must collide to produce the rxn indicated by that step.
Z5e 584
Z5e 585.
i.e., 3 moles of H 2 are being consumed for every 1 mole of N 2
Z5e Fig. 12.1 Definition of Rate Z5e 562
Hrw 532
Fig. 12.13 Z5e 589 (a) and (b) lead to a reaction, but (c) cannot.
Hrw 534
Hrw 534
Hrw 562-563
Vonderbrink PL 17
Hrw 705-707; z5e 1024-1025
Hrw 706; z5e 1024
Hrw 706; z5e 1024-1025
Hrw 707; z5e 1024-1025
Hrw 686; z5e 1083
Hrw 686
Hrw 538
Z5e 559
Hrw 538
Hrw 539
Hrw 539
Hrw 540
Hrw 540
Hrw 540 Section 12.8 Catalysis Z5e 592
Fig. 12.15 Z5e 593
Hrw 541
Hwr 541
Z5e 594
Z5e 598
Hrw 541 Section 12.2 Rate Laws Z5e 564 When fwd & rev rxn rates are equal then no change in conc. of either --> equilibrium Rate = k [H 2 ] m [NH 3 ] n Note: “m” and “n” are not coefficients of the balanced equation
Hrw 541
Hrw 541
“ n” is not the coefficient of the balanced reaction. Rf. Z5e 566
Z5e Fig. 12.1 Definition of Rate Z5e 562
Section 12.3 Determining the Form of the Rate Law Z5e 567
Z5e 568
Hrw 541-542 Z5e 570 SE 1.
Rf. SE 12.1 Z5e 570 Be able to write the rate law (using variables) from the reaction !
Hrw 542-543 Fig. 12.9 Z5e 584 NO 2 + NO 2 ---> NO 3 + NO (k 1 ) NO 3 + CO ---> NO 2 + CO 2 (k 2 ) NO 3 is an intermediate Each rx called an elementary step ; I.e., its rate law can be written from its molecularity Molecularity is defined as the # of species that must collide to produce the rxn indicated by that step.