CHM 121 Lecture Notes - Lecture 7: Homogeneous Catalysis, Chemical Equation, Rate Equation
18 Dec 2016
School
Department
Course
Professor
Document Summary
Write the rate expression for the following reaction: Ch4 (g) + 2o2 (g) co2 (g) + 2h2o (g) Determine the rate law and calculate the rate constant for the following reaction from the following data: s2o8. The reaction 2a b is first order in a with a rate constant of 2. 8 x 10-2 s-1 at 800c. Reaction mechanisms: the overall progress of a chemical reaction can be represented at the molecular level by a series of simple elementary steps, the sequence of elementary steps that leads to product formation is the reaction mechanism. The experimental rate law for the reaction between no2 and co to produce no and co2 is rate = k[no2]2. The reaction is believed to occur via two steps: When the rate determining step cannot be determined, a steady-state approximation is typically used. For this, you must assume that the concentration of all intermediates remains constant. The collision model states that molecules must collide to react.
