CHEM102 Lecture Notes - Lecture 6: Three Steps, Exothermic Process, Activation Energy

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Camille De Browne- Forbes

Document Summary

Step 1: no2 + f2 no2f + f (slow) Step 2: no2 + f no2f (fast) *the structure is like so in this transition state. Step 1: no + o2 no3 (fast) Step 2: no3 + no 2no2 (slow) Fast equilibrium steps relationship with equilibrium constant. The ratio k1 = [c]2 = [products]stoichiometric coefficient k-1 [a][b] [reactants] stoichiometric coefficient. The right hand side of the equation is simply the definition of the equilibrium constant k. Remember: rate constants are given by lower case k and equilibrium constant are given by upper case k. A situation can occur in which either: no information is known or given about the relative speeds of the rates, when steps have relatively comparable rates. If n2o2 is formed in the first step at the same rate it is consumed in the second step the it is steady. Both the reactions have approximately the same rates.