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Discussion on rate of reaction =for quiz 1 and 2

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Discussion on rate of reaction =for quiz 1 and 2

1. 1. what is? Effective collision? Collision theory? Factors affecting? Activation energy? Energy level diagram? Rate of reaction
2. 2. AVERAGE RATE OF REACTION For the whole exp From X min to Y min On the X min (2 nd ) ( from 2 nd to 1 st ) For first x (3) min ( from 0 to 3rd )
3. 3. b) Example from the graph, determine: <ul><li>i) The average rate of reaction for the whole experiment = </li></ul>Total volume of gas Total time taken
4. 4. = 46 = 0.20 cm 3 s -1 210
5. 5. b) Example from the graph, determine: <ul><li>i) The average rate of reaction from 3 minute to 1 minute = </li></ul>Total volume of gas at 3min -1 min Total time taken at 3min -1min
6. 6. = 44-25 = 0.13 cm 3 s -1 180-60
7. 7. b) Example from the graph, determine: <ul><li>i) The average rate of reaction for on the 3 rd minute= </li></ul>Total volume of gas at 3min – at 2min Total time taken at 3min – at 2 min
8. 8. = 44-38 = 0.10 cm 3 s -1 180-120
9. 9. b) Example from the graph, determine: <ul><li>i) The average rate of reaction for for the first 2 minutes= </li></ul>Total volume of gas at 2min – at 0min Total time taken at 2min – at 0 min
10. 10. = 38-0 = 0.33 cm 3 s -1 120-0
11. 11. INSTANTANEOUS RATE OF REACTION ( rate of reaction at that time) Draw tangent to the graph Y X Rate = Y/X
12. 12. b) Example from the graph, determine: <ul><li>i) The rate of reaction at 120 s </li></ul>Instantaneous rate of reaction = Draw tangent to the graph
13. 13. = 56 – 20 = 0.176 cm 3 s -1 222-18
14. 17. II I III Volume of gas Time <ul><li>decrease temperature </li></ul><ul><li>Decrease TSA </li></ul><ul><li>Decrease conc but not the mole of reactant </li></ul><ul><li>Use positive catalyst </li></ul><ul><li>Increase temperature </li></ul><ul><li>Increase total surface area (TSA) </li></ul><ul><li>Increase conc but not the mole of reactant </li></ul>
15. 18. Example: Sketch curve that would be obtained with the changes below: original Lower temp Volume of gas Time Lower temperature is used
16. 19. Example: Sketch curve that would be obtained with the changes below: original higher temp Volume of gas Time Higher temperature
17. 20. Example: Sketch curve that would be obtained with the changes below: original Bigger size Volume of gas Time Bigger size of reactant is used
18. 21. Example: Sketch curve that would be obtained with the changes below: original Smaller size Volume of gas Time Smaller size of reactant
19. 22. Example: Sketch curve that would be obtained with the changes below: original higher temp Volume of gas Time Higher temperature
20. 23. Example: Sketch curve that would be obtained with the changes below: original With catalyst Volume of gas Time Catalyst was added
21. 24. Changes to the FLAT part of graph
22. 25. Example: Curve I represents the result of the experiment using excess zinc powder and 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid I Volume of gas/ cm 3 Time/s
23. 26. Draw curves when condition change: ORIGINAL: 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid Change : 50cm 3 of 2.0 moldm -3 dilute hydrochloric acid ori Volume of gas/ cm 3 Time/s Change
24. 27. Draw curves when condition change: ORIGINAL: 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid Change : 50cm 3 of 0.5 moldm -3 dilute hydrochloric acid ori Volume of gas/ cm 3 Time/s Change
25. 28. Draw curves when condition change: ori :50cm 3 of 1.0 moldm -3 dilute hydrochloric acid change : 50cm 3 of 0.5 moldm -3 dilute hydrochloric acid ori Volume of gas/ cm 3 Time/s change
26. 29. Draw curves when condition change: ORI : 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid change : 20cm 3 of 1.0 moldm -3 dilute hydrochloric acid ori Volume of gas/ cm 3 Time/s change
27. 30. Draw curves when condition change: ori: 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid change: 25cm 3 of 2.0 moldm -3 dilute hydrochloric acid ori Volume of gas/ cm 3 Time/s change
28. 31. 1. The effect of size of reactant <ul><li>Reducing the size of reactant </li></ul><ul><li>increases the Total Surface Area </li></ul><ul><li>increases the frequency of collisions </li></ul><ul><li>between particles </li></ul><ul><li>Increase the rate of reaction . </li></ul><ul><li>Increase the frequency effective </li></ul><ul><li>collisions between particles </li></ul>
29. 32. 2. The effect of temperature <ul><li>Increase the temperature of solution </li></ul><ul><li>increase the kinetic energy of particles </li></ul><ul><li>increase the frequency of collisions </li></ul><ul><li>between particles </li></ul><ul><li>Increase the rate of reaction . </li></ul><ul><li>Increase the frequency effective </li></ul><ul><li>collisions between particles </li></ul>
30. 33. 3. The effect of concentration <ul><li>Increase the concentration of solution </li></ul><ul><li>increase the number of particles per unit volume </li></ul><ul><li>increase the frequency of collisions </li></ul><ul><li>between particles </li></ul><ul><li>Increase the rate of reaction . </li></ul><ul><li>Increase the frequency effective </li></ul><ul><li>collisions between particles </li></ul>
31. 34. 4. The effect of catalyst <ul><li>Catalyst provides alternative route </li></ul><ul><li>That has a lower activation energy </li></ul><ul><li>Increase the rate of reaction . </li></ul><ul><li>So more particles have energy equal or </li></ul><ul><li>greater than activation energy . </li></ul><ul><li>Number of effective collisions increase . </li></ul>
32. 35. exothermic reaction
33. 36. Activation energy with catalyst Activation energy no catalyst reactant
34. 37. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Calcium carbonate and hydrochloric acid ( 2m) </li></ul>
35. 38. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Sodium thiosulphate and sulphuric acid( 2m) </li></ul>
36. 39. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Decomposition of hydrogen peroxide ( 2m) </li></ul>
37. 40. What is the catalyst used in the decomposition hydrogen peroxide?(1m) Manganese (IV) oxide
38. 41. Write ionic equation for Sodium thiosulphate and sulphuric acid (2m)
39. 42. End