![What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] Rate = k [B] 2.0 x 10 – 4 0.20 0.20 1.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] A + 2 B products](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-4-320.jpg)
![What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] Rate = k [B] 2.0 x 10 – 4 0.20 0.20 1.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] A + 2 B products](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-5-320.jpg)
![What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] 2 [B] 4 Rate = k [B] 8.0 x 10 – 4 0.20 0.20 4.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] 2 A + B products](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-6-320.jpg)
![What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] 2 [B] 4 Rate = k [B] 8.0 x 10 – 4 0.20 0.20 4.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] 2 A + B products](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-7-320.jpg)
![What are the units of the rate constant for a reaction with a rate law of: M s M 2 s M – 1 s – 1 M – 1 s – 2 M – 2 s – 1 Rate = k [A][B]](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-8-320.jpg)
![What are the units of the rate constant for a reaction with a rate law of: M s M 2 s M – 1 s – 1 M – 1 s – 2 M – 2 s – 1 Rate = k [A][B]](https://image.slidesharecdn.com/ch14clickerset2-091021104427-phpapp01/85/Ch12-questions-II-9-320.jpg)
Ch12 questions II
- 1. Chapter 14 Chemical Kinetics Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten and Catherine J. Murphy Donna Narsavage Heald Siena College Loudonville, NY 2009, 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? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] Rate = k [B] 2.0 x 10 – 4 0.20 0.20 1.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] A + 2 B products
- 5. What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] Rate = k [B] 2.0 x 10 – 4 0.20 0.20 1.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] A + 2 B products
- 6. What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] 2 [B] 4 Rate = k [B] 8.0 x 10 – 4 0.20 0.20 4.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] 2 A + B products
- 7. What is the rate law for the reaction? Rate = k [A][B] 2 Rate = k [A][B] Rate = k [A] 2 [B] Rate = k [A] 2 [B] 4 Rate = k [B] 8.0 x 10 – 4 0.20 0.20 4.0 x 10 – 4 0.20 0.10 1.0 x 10 – 4 0.10 0.10 Initial Rate M /s [B] [A] 2 A + B products
- 8. What are the units of the rate constant for a reaction with a rate law of: M s M 2 s M – 1 s – 1 M – 1 s – 2 M – 2 s – 1 Rate = k [A][B]
- 9. What are the units of the rate constant for a reaction with a rate law of: M s M 2 s M – 1 s – 1 M – 1 s – 2 M – 2 s – 1 Rate = k [A][B]
- 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? 2 x 500 = 1000 s 3 x 500 = 1500 s 4 x 500 = 2000 s 5 x 500 = 2500 s 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? 2 x 500 = 1000 s 3 x 500 = 1500 s 4 x 500 = 2000 s 5 x 500 = 2500 s 8 x 500 = 4000 s