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Unformatted text preview: Determining Rate Laws Initial Rates MethodDifferential Rates 1. Find two experiments in which all but one reactants concentration is constant. 2. Observe the relationship between concentration change and rate change of that reactant. 3. Repeat for other reactant(s). NH 4 + (aq) + NO 2 (aq) N 2 (g) + 2 H 2 O(l) 5.40 x 107 0.0100 0.200 3 2.70 x 107 0.0100 0.100 2 1.35 x 107 0.0050 0.100 1 Initial Rate (Ms1 ) [NO 2 ] o [NH 4 + ] o Exp. # Determine the rate law Rate = k[NH 4 + ][NO 2 ] Practice Problem Determine the value of the rate constant. 2 NO(g) + Cl 2 (g) 2 NOCl(g) 1.45 0.20 0.20 3 0.36 0.20 0.10 2 0.18 0.10 0.10 1 Initial Rate (Mmin1 ) [Cl 2 ] o [NO] o Exp. # Practice Determine rate law and rate constant BrO 3 (aq) + 5 Br(aq) + 6 H + (aq) 3 Br 2 (l) + 3 H 2 O(l) 3.2 x 103 0.20 0.10 0.10 4 0.20 0.10 0.10 [Br] o 3.2 x 103 0.10 0.20 3 1.6 x 103 0.10 0.20 2 8.0 x 104 0.10 0.10 1 Initial Rate (Ms1 ) [H + ] o [BrO 3 ] o Exp. # Practice Determine rate law and rate constant The Change of Concentration with Time aA products 1 st order y = mx + b Plot: ln[A] vs. t slope = k ] [ ] [ A k t A rate = = o t A kt A ] ln[ ] ln[ + = o t t o A A for kt A A ] [ ] [ , ] [ ] [ ln < = integrate Concentration and time of 1 st order reaction [A] t ln[A] t...
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This note was uploaded on 08/06/2008 for the course CHEM 1B taught by Professor Watts during the Winter '08 term at UCSB.
 Winter '08
 Watts
 Chemistry

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