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Chemical kinetics


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This set of powerpoint slides revolves around the topic of chemical kinetics. Are you looking for notes on factors affecting speed of reaction? Looking for foolproof ways to calculate the rate of reaction? You have come to the right place!
Excellent as a chemistry study material and as an examination revision tool :) A short and sweet O level topic guide with the things you need to ace in chemical kinetics!

Published in: Education, Technology
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Chemical kinetics

  1. 1. Chemical kinetics
  2. 2. Rate of a reaction O 1) amount of reactant used up/time taken O 2) amount of product formed/time taken O 3) volume of gas produced/time taken
  3. 3. Measuring rate of reaction – volume of gas produced O Since magnesium reacts with dilute HCl to form hydrogen gas, the speed of reaction can hence be determined by measuring the volume of hydrogen gas produced at regular time intervals.
  4. 4. Experimentation Time! O Conduct your own experiment and sketch out your own vol. of hydrogen vs time graph!
  5. 5. Graph analysis O Gradient of graph  speed of reaction O The steeper the gradient, the faster the speed of reaction O Decrease in steepness indicates decreasing speed of reaction O Shape of graph  changes/consistency in speed of reaction as time passes
  6. 6. Measuring speed of reactionchanges in mass O Allow gas produced to escape and measure the loss of mass O Reaction speed determined by measuring loss of mass at regular time intervals
  7. 7. Factors affecting rate of a chemical reaction O Summary: O Temperature O Concentration O Pressure O Surface area O Presence of a catalyst
  8. 8. Collision theory O For a reaction to occur, reacting particles must O 1) collide with each other O 2) possess activation energy O Note: Orientation of collision must be correct as well
  9. 9. Factor 1: Temperature O Increase in temp.  increase in KE  increase in no. of collisions + increase in no. of particles with greater than required amount of activation energy  more particles react  increase rate of reaction
  10. 10. Put on your thinking cap! O Can you explain why food should be kept in deep-freeze compartments in order to ensure its freshness? O (answer on next slide)
  11. 11. O Answer: O The low temperature slows down chemical reactions which makes the food turn bad.
  12. 12. Factor 2: Concentration/Pressure O High concentration/pressure  more particles per unit volume  increase in frequency of collisions  rate of reaction increases
  13. 13. Factor 3: Surface area O Increase in surface area/particle size  increase in exposure to the other reactant  increase in probability of collisions  increase in rate of reaction
  14. 14. Factor 4: Presence of Catalyst O Speeds up rate of reaction through lowering activation energy needed for reaction to occur O Think: What can you infer from the above statement?
  15. 15. The end Learn through understanding, not through memorization.