GEN_CHEM_7-KINETICS_&_RX_RATES-2007-WEB

GEN_CHEM_7-KINETICS_&_RX_RATES-2007-WEB - Topic 7...

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Topic 7: Kinetics and Reaction Rates Objectives: By t he end of t his t opic, you should: 1. be f amiliar wit h t he concept s of kinet ic and pot ent ial energy. 2. underst and t he concept of act ivat ion energy, and t he energy needed t o complet e a chemical react ion. 3. underst and t he t erms exot hermic and endot hermic, and be able t o correlat e t hem wit h heat f low bet ween a syst em and it s surroundings. 4. be able t o writ e t he react ion rat e expression f or a simple react ion. 5. underst and t he ef f ect s of t emperat ure, concent rat ions and cat alyst s on react ion rat es. Suggest ed reading: DTC, Chapt er 7, pp. 207-225 Homework problems: 7.33, 7.34, 7.59, 7.60, 7.67, 7.71, 7.72, 7.74 Note: We will begin this topic on Friday, Aug. 31 and finish it on Wednesday, Sept. 5. Bring theseslides to class on Friday
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Kinetics and reaction rates For a chemical Rx to takeplace, molecules of the reactants must contact each other (collide) with enough energy to react and form new bonds . If molecules collide with enough energy to break existing bonds and form new bonds, the chemical Rx will occur. Activation Energy – energy required to break existing bonds and/or form new ones (allow the Rx to take place) If collision energy is less than activation energy, molecules bounce apart without reacting. Kinetics is thestudy of the rate(speed) at which chemical Rx occur. All molecules, ions, and atoms are constantly in motion (except at absolute zero). They move around and collide with each other and with other particles.
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As an example, consider the reaction of carbon (C) and oxygen (O 2 ) to form carbon dioxide (CO 2 ).
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