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# Lecture 4 - 2 NO(g Cl2(g 2 NOCl(g 2 Using method of initial...

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1/13/10 1 28 What is the rate constant k? A) k = 21 B) k = 2.1 ! 10 -2 M -2 s -1 C) k = 21 M s -1 D) k = 21 M -2 s -1 E) k = 2.1 ! 10 -2 M s -2 To find k, use data from any experiment (#1) 0.021 mol/Ls = k (0.100 mol/L) 2 (0.100 mol/L) 1 k = 21 (mol/L) -2 s -1 = 21 M -2 s -1 ***NEVER REPORT k WITHOUT UNITS Rate = k[NO] 2 [Cl 2 ] 2 NO (g) + Cl 2 (g) ! 2 NOCl (g) Rate = k[NO] 2 [Cl 2 ] Using method of initial rates determined 29 Given the rate law and [A] 0 , A ! products Consider the simple reaction: Rate of reaction = ! " [A] " t = k[A] n Given [A] 0 and [A] t , How do you find [A] t ? How do you find the rate law? (i) First-order reaction: ! d[A] dt = k[A] 1 Rate = 1 [A] d[A] = ! kdt Integrate: 1 [A] [ A ] 0 [ A ] t ! d[A] = " kdt 0 t ! ln[A] t - ln[A] 0 = -kt 2.B. Integrated Rate Laws (Section 16.4) - Change form of rate law so that reactant concentration expressed as a function of time For the reaction : A ! products 30 Instantaneous Rearrange: 31 ln[A] t = -kt + ln[A] o ln A [ ] t A [ ] 0 ! " # \$ % = kt

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Lecture 4 - 2 NO(g Cl2(g 2 NOCl(g 2 Using method of initial...

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