CHM 11600 Lecture Notes - Lecture 3: Rate Equation, Kinetic Energy
25 Mar 2015
School
Department
Course
Professor
Document Summary
Chm 11600 - general chemistry - lecture 3_rate laws. 0. 050 (decrease by a quarter as time increases) (halves as time increases) Rate2/rate1 = k[clo2]x[oh-]y/k[clo2]x[oh-]y = [0. 100]x/[0. 050]x = [2]x = 2. 30*10-1/5. 75*10-2 = 4. Solving for k 2. 30*10-1 = k[0. 100]2[0. 100] k = 2. 30*102 m2/s-1. For a zero order reaction: a products, rate = k. The integrated rate law is [a] = -kt + [ao] For a first order reaction: a products, rate = k[a] The integrated rate law is ln [a] = -kt + ln [ao] For a second order reaction: 2a products or a + b products (when [a] = [b]), rate = k[a]2. The integrated rate law is 1/[a] = kt + 1/[ao] Rate is proportional to # of collisions between reactant species / time. Experimentally: only a small fraction of collisions produce a reaction. Activation energy (ea) must be overcome to produce a chemical reaction.
