CHEM102 Lecture Notes - Lecture 3: Rate Equation, Reaction Rate Constant, Third Order

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Sai Yiu

Document Summary

Rate(4) 1. 65 x 10-5 k (0. 100)n (0. 300)m rate(5) 3. 30 x 10-5 k (0. 100)n (0. 600)m. = (0. 500) m (0. 500) m = 0. 500 m = 1 k = 5. 50 x 10-3 m-2 s-1 rate (1) = k (0. 100 m)2 (0. 100 m) = 5. 50 x 10-6 m s-1. **note that the unit of k is dependent on overall orders. Thus the reaction is first order for b and second order for a and the overall order of reaction is 1 + 2 = 3. We say that it is a third order reaction. 1 the following is the data of a reaction at 800oc. Determine the rate law and the rate constant of the reaction. Initial [no] (m) initial rate (m / min) Rate of reaction = k [h2]n[no]m rate(1) 4. 2 x 10-3 k (0. 50)n (1. 50)m rate(2) 1. 3 x 10-2 k (1. 50)n (1. 50)m. 1. 50 1. 3 x10-2 (0. 333) n = 0. 323 n = 1 rate(2) 1. 3 x 10-2 k (1. 50) (1. 50)m.