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Lecture%2023%20April%209%20%28Chapter%2016%20--%20Kinetics%29

# Lecture%2023%20April%209%20%28Chapter%2016%20--%20Kinetics%29

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Chapter 16 -- Kinetics Lecture 23 April 9, 2009

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Reaction Rates and Temperature

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Example: Cyclobutane decomposes to form ethylene C 4 H 8 2C 2 H 4 Experimental rate constants for this reaction are k = 6.1 x 10 -8 s -1 at 327 o C and k = 1.5 x 10 -4 s -1 at 245 o C. Determine E a .

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Example: For a certain reaction the rate constant doubles when the temperature is increased from 15-25 o C. Calculate the activation energy for the reaction and the rate constant at 100 o C if k at 25 o C is 1.2 x 10 -2 L mol - 1 s -1 .

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The Arrhenius equation, k = Ae -(Ea/RT) , expresses the relationship between the reaction rate constant, k, and the energy of activation, E a . The probability that

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Unformatted text preview: colliding molecules will react (A) increases with increasing energy of activation (A) depends only on the empirical constant A (A) increases with decreasing temperature (A) decreases with increasing energy of activation Substance A undergoes a first order reaction, A B, with a half life of 20 minutes at 25 o C. If the initial concentration of A is 1.6M, what will be the concentration of A after 80 minutes? (A) 0.40M (A) 0.20M (A) 0.10M (A) 0.050M hich line in the diagram represents the activation energy for a forward reaction? A B C D - E reaction coordinate → (A) A (B) B (C) C (D) D...
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Lecture%2023%20April%209%20%28Chapter%2016%20--%20Kinetics%29

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