603Theory

603Theory - Collision theory of gaseous reactants For the...

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1 Lesson 28 Collision theory of gaseous reactants For the bimolecular elementary reaction, A + B products to occur, it is necessary that molecules of A and B collide. Will all colliding molecules react? The rate of molecular collisions per volume can be estimated by the expression: V N V N u s cm collision . No B A 2 3  Lesson 28 Calculating the frequency of collisions in a gas reaction At 1 atm and 0 o C, assuming ideal gas behaviour, some typical values are: s cm u cm cm V N V N B A 4 8 3 19 10 5 10 3 10 8 . 2 s cm collisions s cm collision No 3 29 3 10 1 . 1 . Molecular density: Molecular radius: Average speed: A very high frequency! Lesson 28 Activation energy • If molecular collisions were the only controlling factor for chemical reactions taking place in the gas phase, this very high rate of molecular collisions would indicate that all gas reactions would be extremely fast. This does not agree with experimental data on gas reactions. • In fact, reactant molecules must achieve a given
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This note was uploaded on 11/29/2011 for the course CHE 102 taught by Professor Simon during the Fall '08 term at Waterloo.

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603Theory - Collision theory of gaseous reactants For the...

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