Rates of Reaction From Method of Initial Rates

Rates of Reaction From Method of Initial Rates to Integrated Rate Law

Method of Initial Rates The initial rates listed in the following table were determined for the reaction: 2 NO(g) + Cl 2(g) 2 NOCl(g) Experiment Initial [NO] (M) Initial [Cl 2] (M) 1 2 3 0. 13 0. 26 0. 13 0. 20 0. 10 Initial Rate of Consumption of Cl 2 (M/s) 1. 0 × 10 -2 4. 0 × 10 -2 5. 0 × 10 -3 1. What is the order of the reaction with respect to each reactant? 2. What is the rate law? 3. What is the value of the rate constant?

Time (s) 0 50 100 200 400 [N 2 O 5] (M) 0. 1000 0. 0707 0. 0500 0. 0250 0. 00625 Integrated Rate Laws N 2 O 5 (g) 2 NO 2 (g) + ½ O 2 (g) 1. What is the order of the reaction with respect to each reactant? 2. What is the rate law? 3. What is the value of the rate constant?

Integrated Rate Laws •

Rate = k Integrated Rate Laws Second Order Zero Order First Order The graph that is linear indicates the order of the reaction with respect to A.

Rate = k[A] Integrated Rate Laws Second Order Zero Order First Order The graph that is linear indicates the order of the reaction with respect to A.

Integrated Rate Laws Rate = k[A]2 Second Order Zero Order First Order The graph that is linear indicates the order of the reaction with respect to A.

Integrated Rate Law: Summary Table First Order Rate Law Concentration-Time Equation Linear Graphical Determination of k Half-Life Equation Second Order

Integrated Rate Law: Summary Table First Order Second Order Rate Law Concentration-Time Equation ln[R]t = -kt + ln[R]o Linear Graph ln[R] vs. t Graphical Determination of k k = -slope Half-Life Equation k = slope