Kinetics

Oct 20, 2012

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What is Kinetics ?. Analysis of reaction mechanisms on the molecular scaleDerivation of rate expressionsDesign and analysis of experiments to test rate equations and derive kinetic parameters Theoretical prediction of rate constantsHow can we improve it?. Elementary steps. Di

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Kinetics

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Kinetics

Kinetics. The Rates and Mechanisms of Chemical Reactions. SC4. Obtain, evaluate, and communicate information about how to refine the design of a chemical system by applying engineering principles to manipulate the factors that affect a chemical reaction.

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Kinetics

Kinetics. Collision Theory: How reactions takes place. Why are kinetics important?. In order to control processes. speed up useful reactions that occur to slowly slow down reactions that are harmful Example:

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Kinetics

Kinetics. Advanced Higher Chemistry Unit 2(f). The Rate Law. a A + b B → c C + d D. Rate  [A] m .[B] n. Rate = k [A] m .[B] n. Where… k = rate constant m and n = orders of reaction with respect to A and B. Orders of reaction.

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Kinetics

Kinetics. Ch 15. Kinetics. Thermodynamics and kinetics are not directly related Investigate the rest of the reaction coordinate Rate is important!. Chemical Kinetics. Kinetics – the study of the rates of chemical reactions

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Kinetics

Kinetics. The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can’t tell how fast. Diamond will spontaneously turn to graphite – eventually. Reaction mechanism- a series of steps by which a reaction takes place. Reaction Rate.

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Kinetics

Kinetics. Chapter 12 Chemistry SC5. Think About It. Rank in order from slowest to fastest chance of causing an automobile accident. Option A : A person obeying all the traffic laws Option B : A person changing the radio station in the car.

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Kinetics

Kinetics. Ways to Express Rates. Relative Average Instantaneous. More commonly, rates are expressed by a rate law or rate expression – two methods: Differential – expresses how rate depends on initial concentration Integrated – expresses how concentration depends on time.

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Kinetics

Kinetics. Rates of Reaction. Faster only means faster. It doesn’t mean bigger It doesn’t mean more of the product It only means the rxn is completed faster, the reactants are turned into products in less time. Not a reaction but think about it.

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Kinetics

Kinetics. Answers question, “How fast?” Rate is proportional to the concentration of reactants raised to a power. Rate law is experimentally determined. =>. =>. Activation Energy. Minimum energy required to reach the transition state .

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Kinetics

Kinetics. The Study of Rates of Reaction. Rate of a Reaction. The speed at which the reactants disappear and the products are formed determines the rate of the reaction. The reaction rate slows as the concentration of the reactants decrease and the concentration of the products increases.

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Kinetics

Kinetics. The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can’t tell how fast. Reaction mechanism- the steps by which a reaction takes place. Reaction Rate. Rate = Conc. of A at t 2 -Conc. of A at t 1 t 2 - t 1 Rate = D [A] D t

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Kinetics

Kinetics. 2000D By: Charles Liao. 2000D. a. Referring to the data in the table below, calculate the standard enthalpy change, for the reaction at 25 ˚C. O 3(g) + NO (g)  O 2(g) + NO 2(g) ∆H =33 (kJ mol-1) -(143+90) (kJ mol-1) =-200 (kJ mol-1). 2000D.

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Kinetics

Kinetics. Reaction rate and rate laws. Reaction rate: rate = Δ concentration of species Δ t aA + bB → cC + dD rate = Δ[C] = Δ[D] = -Δ[A] = - Δ[B] c Δ t d Δ t a Δ t b Δ t. Dependence on concentration of reactants: single reactant, A:

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Kinetics

Kinetics. The study of reaction rates. Spontaneous reactions are reactions that will happen - but we cannot tell how fast. Diamond will spontaneously turn to graphite – eventually. Reaction mechanism- the steps by which a reaction takes place. Reaction Rate.

973 views • 82 slides

Kinetics

Kinetics. From properties of materials to Reaction Chemistry. 2 levels of study, for 2 reasons:. Macroscopic view: How fast? Rates of reaction typically as D concentration per time. Microscopic view: What path? Mechanism sequence of chemical steps, to control it.

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kinetics

kinetics. Collision Theory. Reactants must collide with proper orientation and sufficient energy. Transition State Theory . Explains what happens once colliding particles react Transition state is the in-between state when reactants are being converted to products

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Kinetics

Kinetics. What is Kinetics ?. Analysis of reaction mechanisms on the molecular scale Derivation of rate expressions Design and analysis of experiments to test rate equations and derive kinetic parameters Theoretical prediction of rate constants How can we improve it?.

900 views • 38 slides

Kinetics

Kinetics. Click to start. The rate increases with time because the acid becomes more dilute. The rate decreases with time because the acid becomes more dilute. A. B. The rate decreases with time because the magnesium carbonate particls get smaller.

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Kinetics

Kinetics. Patrick Cable, Dat Huynh, Greg Kalinyak, Ryan Leech, Wright Makambi, Ronak Ujla. Batch Reactor. No inlet or outlet flow Reactants are placed inside the reactor and allowed to react over a set period of time Advantages High Conversion can be achieved if allowed a long reaction time

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KINETICS

KINETICS. How Fast Does A Reaction Occur?. Energy Diagrams. Reactants always start a reaction so they are on the left side of the diagram. Products are on the right. Reactants. Products. Exothermic Reactions.

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Kinetics

Kinetics. Reaction Mechanism Chapter 14 part V. Reaction Mechanisms. The steps that add up to the overall balanced reaction equation. May be simple with 2 or 3 steps or very complicated in reactions that may take many steps.

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Kinetics

Kinetics. Unit 6. Video AP 6.1. Rate Expression. Objectives. You should already be able to… Explain collision theory. Describe the rate of a reaction. Describe what factors affect the rate. By the end of the video you should be able to… Write the rate expression for a reaction.

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