Lecture 4 - 1/13/10 2 NO (g) + Cl2 (g) ! 2 NOCl (g) 2 Using...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
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
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 3

Lecture 4 - 1/13/10 2 NO (g) + Cl2 (g) ! 2 NOCl (g) 2 Using...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online