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- 1. what is? Effective collision? Collision theory? Factors affecting? Activation energy? Energy level diagram? Rate of reaction
- 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. 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. = 46 = 0.20 cm 3 s -1 210
- 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. = 44-25 = 0.13 cm 3 s -1 180-60
- 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. = 44-38 = 0.10 cm 3 s -1 180-120
- 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. = 38-0 = 0.33 cm 3 s -1 120-0
- 11. INSTANTANEOUS RATE OF REACTION ( rate of reaction at that time) Draw tangent to the graph Y X Rate = Y/X
- 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. = 56 – 20 = 0.176 cm 3 s -1 222-18
- 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>
- 18. Example: Sketch curve that would be obtained with the changes below: original Lower temp Volume of gas Time Lower temperature is used
- 19. Example: Sketch curve that would be obtained with the changes below: original higher temp Volume of gas Time Higher temperature
- 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
- 21. Example: Sketch curve that would be obtained with the changes below: original Smaller size Volume of gas Time Smaller size of reactant
- 22. Example: Sketch curve that would be obtained with the changes below: original higher temp Volume of gas Time Higher temperature
- 23. Example: Sketch curve that would be obtained with the changes below: original With catalyst Volume of gas Time Catalyst was added
- 24. Changes to the FLAT part of graph
- 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
- 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
- 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
- 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
- 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
- 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
- 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>
- 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>
- 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>
- 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>
- 35. exothermic reaction
- 36. Activation energy with catalyst Activation energy no catalyst reactant
- 37. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Calcium carbonate and hydrochloric acid ( 2m) </li></ul>
- 38. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Sodium thiosulphate and sulphuric acid( 2m) </li></ul>
- 39. <ul><li>Write chemical equation ( 9m) </li></ul><ul><li>Decomposition of hydrogen peroxide ( 2m) </li></ul>
- 40. What is the catalyst used in the decomposition hydrogen peroxide?(1m) Manganese (IV) oxide
- 41. Write ionic equation for Sodium thiosulphate and sulphuric acid (2m)
- 42. End

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