CHE-1102 Lecture Notes - Lecture 4: Rate Equation, Reaction Rate, Kinetic Energy
Document Summary
The speed (or rate) at which a reaction takes place. 2 ways to measure the rate of any reaction: Measure the increase in [products] over time. Measure the decrease in [reactants] over time. Measure a change in concentration per change in time. Rate = [ ] / t, where [ ] is the molar concentration. [products] / t slope is + [reactants] / t slope is - By convention, all rates are reported as positive values. A negative sign indicates that the reactant is being lost. The best indicator of the rate of a reaction is the instantaneous rate near the beginning of the reaction. C4h9cl + h2o c4h9oh + hcl. In this reaction, the ratio of c4h9cl to c4h9oh is 1:1 so the rate of disappearance is the same as the rate of appearance. H2o increases at a rate of 2. 0 x 10-4 m/sec as. H2o2 decreases at a rate of 2. 0 x 10-4 m/sec.
