Reaction Kinetics PDF
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This presentation provides an overview of reaction kinetics, covering important concepts like reaction rates, rate laws, and half-lives. It includes examples and explanations for zero-order, first-order, and second-order reactions.
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Reaction Kinetics Two important terms in reaction: Thermodynamics: Does a reaction take place? Kinetics How fast does a reaction proceed? t is the application of reaction kinetic harmacy? Reaction Rates Rates of reactions can be determined by monitorin...
Reaction Kinetics Two important terms in reaction: Thermodynamics: Does a reaction take place? Kinetics How fast does a reaction proceed? t is the application of reaction kinetic harmacy? Reaction Rates Rates of reactions can be determined by monitoring the change in concentration of either reactants or products as a function of time t. Reaction rate A B D[A] rate = - Dt D[B] rate = Dt Rate law Rate = k [A]m [B]n - [A] & [B] represent the reactants. - The exponents m and n are called “reaction orders”. - The proportionality constant k is called the rate constant. - The overall reaction order is the sum of the reaction orders. – - The overall “order of reaction” is therefore… m + n + …. Zero order reaction The velocity is seen to be constant and independent of.the concentration of the reactants ]A0[ Slope= -K First order reaction Second order reaction Half-life The time required for a quantity to reduce to half its initial value Zero order reaction (half life) First order reaction (half life) Second order reaction (half life)
