012309 - Reactions with More Than One Reactant For the...

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Reactions with More Than One Reactant y For the reaction: { BrO 3 - (aq) + 5 Br - (aq) + 6 H + (aq) 3 Br 2 (l) + 3 H 2 O (l) y Rate = - [BrO 3 - ]/ t = k[BrO 3 - ][Br - ][H + ] 2 y to find k, take an experiment where the concentrations of two of the reactants are much higher than the other reactant, can find k’ and solve for k
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Reactions with More Than One Reactant y For the reaction: { BrO 3 - (aq) + 5 Br - (aq) + 6 H + (aq) 3 Br 2 (l) + 3 H 2 O (l) y Rate = - [BrO 3 - ]/ t = k[BrO 3 - ][Br - ][H + ] 2 y find k when [H + ] o = 1.00 x 10 -4 M, [Br - ] o = [BrO 3 - ] = 0.500 M and after 9.5 s [H + ] = 5.00 x 10 -5 M
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Integrated Rate Law: Summary
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Iodine Clock Reaction 15.0 12.5 10.0 7.5 5.0 mL NaIO 3 Time (s) ln (mL NaIO 3 ) 1/(mL NaIO 3 )
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What do you think is the order of the iodine clock reaction? 0 1 2 3% 14% 82% 1. 0 2. 1 3. 2
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Rate Definition
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Rate Definition
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Reaction Mechanism y Reaction Mechanism – the series of steps taken for a reaction to take place y Intermediate – any substances that is produced in one step and consumed in a later step and does not appear in the overall reaction y Molecularity – the number of molecules that must collide to produce the given reaction
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Reaction Mechanism y Elementary Steps – steps whose rate law can be written from their balanced molecular equation
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