6.1.3 Factors affecting rate of reaction

• What is the relationship between temperature, kinetic energy, collisions, and reaction rate?

  • High temperature: High kinetic energy
  • More frequent and forceful collisions
  • Faster reaction rate
  • Low temperature: Low kinetic energy
  • Less frequent and gentle collisions
  • Slower reaction rate
• Why does higher temperature increase reaction rates?

  Molecules have more kinetic energy
• What is the relationship between concentration and reaction rate?

  • Higher concentration = more reactant molecules
  • More reactant molecules = more frequent collisions
  • More collisions = increased chance of successful reactions
• How does higher concentration affect the rate of reaction?

  It speeds up the rate of reaction
• What is the effect of low concentration on collision frequency?

  It leads to less frequent collisions
• How does increased kinetic energy affect molecular movement?

  Molecules move faster
• Why does increasing concentration lead to more successful reactions?

  More collisions between molecules occur
• What happens to the number of reactant molecules at high concentration?

  There are more reactant molecules
• Why is measuring the rate of reaction important?

  It helps understand the speed of chemical processes
• How can you visualize the role of a catalyst in a reaction?

  Like a key that unlocks a door
• What happens to the reaction rate when temperature increases?

  The reaction speeds up
• How is a catalyst involved in a reaction?

  Not involved
• What are catalysts?

  Substances that speed up reactions
• According to the graph, does a smaller surface area lead to a faster or slower initial reaction rate?


  Slower
• How does cooking illustrate the effect of temperature on reaction rates?

  • Food cooks faster in a hot oven
  • Higher temperature increases reaction rates
  • Lower temperature slows down cooking
• What is the relationship between collision frequency and reaction rate?

  More frequent collisions lead to faster reactions
• What is the result of faster molecular movement?

  More frequent and forceful collisions
• What are the differences between catalyzed and uncatalyzed reactions?

  • Catalyzed Reaction:
  • Rate: Faster
  • Activation Energy: Lower
  • Catalyst Usage: Not Consumed
  • Uncatalyzed Reaction:
  • Rate: Slower
  • Activation Energy: Higher
  • Catalyst Usage: Not Involved
• According to the graph, does a greater surface area lead to a faster or slower initial reaction rate?

  Faster
• What does the rate of reaction indicate?

  How quickly a chemical reaction happens
• What is the rate of reaction when baking a cake that takes 30 minutes?

  1 cake per 30 minutes
• How does surface area influence reaction rate?

  It changes the number of available sites for collisions
• Which line on the graph represents a smaller surface area, such as lumps?

  The lower line
• Why do powders react faster than lumps?

  They have greater surface area for reactions
• What is plotted on the x-axis of the graph?

  Time from start of reaction
• How do stronger collisions affect molecular reactions?

  They make it easier for molecules to react
• How can we measure the rate of reaction?

  By tracking reactants used and products made
• What is the activation energy in a catalyzed reaction compared to an uncatalyzed reaction?

  Lower
• What happens to the reaction rate when surface area increases?

  It increases
• According to the image, what is plotted on the y-axis?

  Total mass / volume of product
• How does the surface area affect the total mass/volume of the product over time?

  • Greater surface area (e.g. powder): Reaches a higher total mass/volume of product in a shorter time.
  • Smaller surface area (e.g. lumps): Reaches a lower total mass/volume of product in a longer time.
• What does concentration refer to in a solution?

  Amount of reactants present
• What does the table summarize about concentration and reaction rates?

  • High concentration: More molecules, more collisions, faster rate
  • Low concentration: Fewer molecules, less collisions, slower rate
• How do catalysts affect chemical reactions?

  They speed up reactions without being consumed
• How can you visualize the effect of concentration on reactions?

  • Imagine a classroom with students
  • More students = more chances for interactions
  • Higher concentration = more chances for reactions
• Which line on the graph represents a greater surface area, such as a powder?

  The upper line
• What is the rate of a catalyzed reaction compared to an uncatalyzed reaction?

  Faster
• What does surface area affect in a reaction?

  Reaction rate
• How does the number of reactant molecules relate to reaction rate?

  More molecules lead to a faster reaction rate
• How is a catalyst used in a reaction?

  Not consumed