Presentation is loading. Please wait.

Presentation is loading. Please wait.

Chapter 15 Chemical Kinetics Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Donna Narsavage.

Similar presentations


Presentation on theme: "Chapter 15 Chemical Kinetics Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Donna Narsavage."— Presentation transcript:

1 Chapter 15 Chemical Kinetics Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Donna Narsavage Heald Siena College Loudonville, NY  2006, Prentice Hall

2 Which expression correctly states the rate of reaction? N 2 (g) + 3 H 2 (g) 2 NH 3 (g)

3 Which expression correctly states the rate of reaction? N 2 (g) + 3 H 2 (g) 2 NH 3 (g)

4 What is the rate law for the reaction? 1.Rate = k[A][B] 2 2.Rate = k[A][B] 3.Rate = k[A] 2 [B] 4.Rate = k[A] 5.Rate = k[B] [A][B]Initial Rate M/s 0.10 1.0 x 10 -4 0.100.201.0 x 10 –4 0.20 2.0 x 10 –4 A + 2 B products

5 What is the rate law for the reaction? 1.Rate = k[A][B] 2 2.Rate = k[A][B] 3.Rate = k[A] 2 [B] 4.Rate = k[A] 5.Rate = k[B] [A][B]Initial Rate M/s 0.10 1.0 x 10 -4 0.100.201.0 x 10 –4 0.20 2.0 x 10 –4 A + 2 B products

6 What is the rate law for the reaction? 1.Rate = k[A][B] 2 2.Rate = k[A][B] 3.Rate = k[A] 2 [B] 4.Rate = k[A] 2 [B] 4 5.Rate = k[B] [A][B]Initial Rate M/s 0.10 1.0 x 10 -4 0.100.204.0 x 10 -4 0.20 8.0 x 10 -4 2 A + B products

7 What is the rate law for the reaction? 1.Rate = k[A][B] 2 2.Rate = k[A][B] 3.Rate = k[A] 2 [B] 4.Rate = k[A] 2 [B] 4 5.Rate = k[B] [A][B]Initial Rate M/s 0.10 1.0 x 10 -4 0.100.204.0 x 10 -4 0.20 8.0 x 10 -4 2 A + B products

8 Rate = k[A][B] What are the units of the rate constant for a reaction with a rate law of: 1. M s 2. M 2 s 3. M -1 s -1 4. M -1 s -2 5. M -2 s -1

9 Rate = k[A][B] What are the units of the rate constant for a reaction with a rate law of: 1. M s 2. M 2 s 3. M -1 s -1 4. M -1 s -2 5. M -2 s -1

10 If t 1/2 = 500 s for a first-order reaction, how long will it take for the concentration of a reactant to decrease to 1/8 of its original value? 1.2 x 500 = 1000 s 2.3 x 500 = 1500 s 3.4 x 500 = 2000 s 4.5 x 500 = 2500 s 5.8 x 500 = 4000 s

11 If t 1/2 = 500 s for a first-order reaction, how long will it take for the concentration of a reactant to decrease to 1/8 of its original value? 1.2 x 500 = 1000 s 2.3 x 500 = 1500 s 3.4 x 500 = 2000 s 4.5 x 500 = 2500 s 5.8 x 500 = 4000 s


Download ppt "Chapter 15 Chemical Kinetics Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Donna Narsavage."

Similar presentations


Ads by Google