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Rate of reaction =measure rate and intro and collision theory
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Rate of reaction =measure rate and intro and collision theory

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  • 1. HOW TO DETERMINE RATE OF REACTION FROM GRAPH AVERAGE RATE OF REACTION INSTANTANEOUS RATE OF REATION
  • 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. INSTANTANEOUS RATE OF REACTION ( rate of reaction at that time) Draw tangent to the graph Y X Rate = Y/X
  • 4. b) Example from the graph, determine:
    • i) The rate of reaction at 120 s
    Instantaneous rate of reaction = Draw tangent to the graph
  • 5. = 56 – 20 = 0.176 cm 3 s -1 222-18
  • 6. Changes to the graph
  • 7. Changes to the CURVE part of graph II I III Volume of gas Time Use negative catalyst Decrease temperature Decrease TSA
    • Use positive catalyst
    • Increase temperature
    • Increase total surface area
  • 8. Changes to the FLAT part of graph
  • 9. d) Curve I represents the result of the experiment using excess zinc powder and 50cm 3 of 1.0 moldm -3 dilute hydrochloric acid II I III Volume of gas/ cm 3 Time/s
    • Use positive catalyst
    • Increase temperature of reactant
    Lower concentration of hydrochloric acid
  • 10. Collision theory
    • Theory that explains how factors affect rate of reaction
    • Before reaction can occur, particles must first collide
    • Particles collide so that bonds are broken and new bonds can form
  • 11. Collision theory
    • Collision of particles must be effective collisions to produce result
    • Effective collisions are collisions which
      • produce enough energy to overcome energy of activation
      • correct orientation
  • 12. Collision theory
    • Activation energy is the minimum energy the colliding particles must overcome so that reaction occur
    • In order for particles to overcome the activation energy, several factors involve
  • 13. How factors affect rate of reaction according to collision theory
    • Size of reactant for solid reactant
    • Temperature of reactant mixture
    • Concentration of solution reactant
    • Presence of catalyst
  • 14. How Collision theory explain factor of size of solid reactant
    • The smaller the size of reactant , the larger the total surface area
    • Frequency of Collisions between particles increase
    • Frequency of Effective collisions between particles increase
    • Therefore rate of reaction also increase
  • 15. How Collision theory explain factor of concentration
    • The higher the concentration of reactant solution , the higher the number of particles per unit volume
    • Frequency of Collisions between particles increase
    • Frequency of Effective collisions between particles increase
    • Therefore rate of reaction also increase
  • 16. How Collision theory explain factor of temperature
    • The higher the temperature of reactant solution , the higher the kinetic energy of particles
    • Frequency of Collisions between particles increase
    • Frequency of Effective collisions between particles increase
    • Therefore rate of reaction also increase
  • 17. Collision theory explain factor of catalyst
    • Presence of catalyst provide an alternative path
    • This alternative path has a lower activation energy
    • More colliding particles can overcome this lower activation energy
    • Frequency of Effective collisions between particles increase
    • Therefore rate of reaction also increase