Chem 0120 1st Edition Lecture 6 Outline of Last Lecture I Expressing Rates of Reactions II Integrated Rate Laws III Example 13 5 IV Half Life V Elementary Reactions Outline of Current Lecture I Elementary Reaction II Exercise 13 8 III Mechanism with initial fast step generates intermediate IV Rate Discovery Step R D S V Elementary Reaction VI Equilibrium Current Lecture I Elementary Reaction NO2 g CO g NO g CO2 g Step 1 NO2 NO2 NO3 NO Step 2 NO3 CO NO2 CO2 NO3 is a reaction intermediate formed in one step consumed in another II Exercise 13 8 Rate Law and Mechanism 2H2O2 2H2O O2 Step 1 H2O2 I H2O IOStep 2 H2O2 IO H2O O2 ICatalyst IReaction Intermediate IO III Mechanism with initial fast step generates intermediate These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute 2N2O5 g 4NO2 g O2 g Step 1 N2O5 NO2 NO3 Step 2 NO2 NO3 Step 3 IV Rate Discovery Step R D S Rate k NO2 NO3 rate forward rate reversed at equilibrium R D S in fast step 1 k 1 N 2 O5 K 1 NO 3 NO2 K 1 N 2O 5 NO 3 K 1 NO 2 R D S in slow step 2 Rate K 2 NO 2 NO3 KK2 1K 1 N 2O NO5 2 NO 2 K N O Rate V VI 2 5 Elementary Reaction OH CH3Cl CH3OH Cl2nd Order Biomolecular Nucleophobic Substitution SN Rate k CH3Cl OH Equilibrium Chapter 14 Due to formatting a two way arrow indicating the reaction occurring in both directions will be written as such please do not write like this on exams or homework because it indicates something different which will be taught in later sections Rate of Forward Reaction Rate of Reverse Reaction aA bB cC dD Kc C c D d a b A B Kc is obtained from rate constant at every step of mechanism