89.6 Rate Theories of elementary reaction for bimolecular reaction--simple collision theory SCT cG→Qo Extensive reading: Levine, pp. 879-881
§9.6 Rate Theories of elementary reaction for bimolecular reaction—simple collision theory SCT Extensive reading: Levine, pp. 879-881
89.6 Rate Theories of elementary reaction Two important empirical rules Rate equation(law of mass action)r=kAIB] A rrhenIus equation k=Aexp RT Type of Unimolecular Bimolecular Termolecular reaction reaction reaction reaction 101 10 moIl·dm3s mor.dm.s A seems related to collision frequency. E exp Boltzmann distribution term RT
Two important empirical rules: Rate equation (law of mass action) Arrhenius equation = − RT E k A a exp Type of reaction Unimolecular reaction Bimolecular reaction Termolecular reaction A 1013 s 1011 mol-1 dm3 s -1 109 mol-2 dm6 s -1 A seems related to collision frequency. − RT Ea exp Boltzmann distribution term r k = [A][B] §9.6 Rate Theories of elementary reaction
89.6 Rate Theories of elementary reaction Basic considerations and brief history a molecule of a cannot react with a molecule of b unless the two reactant molecules can somehow interact This interaction can only take place if they come within a certain distance of each other i e. collides with each other Therefore the rate constant of the reaction may be predicted by calculation of the collision frequency of the reactants Collision theory is proposed independently by Max Trautz in 1916 and william Lewis in 1918. Thereafter. C. Hinshelwood made modification on it http:/en.wikipediaorg/wiki/collision_theoR
A molecule of A cannot react with a molecule of B unless the two reactant molecules can somehow interact. This interaction can only take place if they come within a certain distance of each other, i.e., collides with each other. Therefore, the rate constant of the reaction may be predicted by calculation of the collision frequency of the reactants. Collision theory is proposed independently by Max Trautz in 1916 and William Lewis in 1918. Thereafter, C. Hinshelwood made modification on it. Basic considerations and brief history http://en.wikipedia.org/wiki/Collision_theory §9.6 Rate Theories of elementary reaction
89.6 Rate Theories of elementary reaction Basic consideration and brief history Das gesetz der Reaktionsgeschwindigkeit und der Gleich gewichte in Gasen. Bestatigung der Additivitat von Cv-3/2R. Neue Bestimmung der Integrationskonstanten und der Molekildurchmesser Von MAX TRAUTz 2=4y2R丌·A·Vr M+M z. norg. Chem 94(1916)79
Basic consideration and brief history Z. anorg. Chem. 94 (1916), 79 §9.6 Rate Theories of elementary reaction
89.6 Rate Theories of elementary reaction 9.6.1 Fundamental assumptions of Sct For gaseous bimolecular reaction 1) The reaction rate is proportional to the collision frequency(2 which can be solved by kinetic theory of molecule 2) The collision can be either non-reactive(elastic) collision or reactive collision Only the molecules posses energy excess to a critical value (E] can lead to reactive collision. The reaction rate should be in proportion to the fraction of reactive collision(q reaction rate can be expressed as ABg where Zab is the collision frequency of a with B per unit cubic meter per second, q is the portion of effective collision
9.6.1 Fundamental assumptions of SCT For gaseous bimolecular reaction 1) The reaction rate is proportional to the collision frequency (Z) which can be solved by kinetic theory of molecule; AB r Z q = where ZAB is the collision frequency of A with B per unit cubic meter per second, q is the portion of effective collision. reaction rate can be expressed as: 2) The collision can be either non-reactive (elastic) collision or reactive collision. Only the molecules posses energy excess to a critical value (Ec ) can lead to reactive collision. The reaction rate should be in proportion to the fraction of reactive collision (q). §9.6 Rate Theories of elementary reaction