070808 - y Elementary Steps Reaction Mechanism y Two...

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2 nd Order Reaction
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Half-Life of a 2 nd Order Reaction
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2 nd Order Reaction y Butadiene (C 4 H 6 ) reacts with itself to form a dimer with the formula C 8 H 12 . The reaction is second order in C 4 H 6 . The rate constant at a particular temperature is 4.0 x 10 -2 M -1 s -1 and the initial concentration of C 4 H 6 is 0.200 M. { What is the molarity of butadiene after a reaction time of 1.00 h?
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2 nd Order Reaction y What is the time (in hours) when the C 4 H 6 concentration reaches a value of 0.0020 M?
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2 nd Order Reaction y What is the half life of the reaction? y How many minutes will it take for the concentration of C 4 H 6 to drop from 0.0100 M to 0.0050 M?
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Zero Order Reaction
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Half-Life for a Zero Order Reaction
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Reactions with More Than One Reactant
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Pseudo-1 st Order Reactions
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Integrated Rate Law: Summary
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Rate Definition 17.5 15 12.5 10.0 7.5 mL NaIO 3 Time (s) ln (mL NaIO 3 ) 1/(mL NaIO 3 )
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Rate Definition
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Rate Definition
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Reaction Mechanism y Reaction Mechanism – y Intermediate – y Molecularity –
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Reaction Mechanism
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Unformatted text preview: y Elementary Steps Reaction Mechanism y Two conditions must be satisfied to have an appropriate reaction mechanism. Reaction Mechanism y Consider the following mechanism for the reaction of hydrogen with iodinemonochloride: y Step 1: H 2 (g) + ICl (g) HI (g) + HCl (g) y Step 2: HI (g) + ICl (g) I 2 (g) + HCl (g) y Write the equation for the overall reaction. y Identify any reaction intermediates. y What is the molecularity of each elementary step? Reaction Mechanism y The balanced equation for the reaction of the gases nitrogen dioxide and fluorine is: { 2 NO 2 (g) + F 2 (g) 2 NO 2 F (g) y The experimentally determined rate law is: { Rate = k[NO 2 ][F 2 ] y A suggested mechanism for this reaction is: { Step 1: NO 2 (g) +F 2 (g) NO 2 F (g) + F (g) Slow { Step 2: F (g) + NO 2 (g) NO 2 F (g) Fast y Is this an acceptable mechanism?...
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070808 - y Elementary Steps Reaction Mechanism y Two...

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