2.2.1 Factors Affecting Rate

• Effective collisions have correct orientation and sufficient energy to overcome activation energy

  True
• A higher concentration of reactants leads to more frequent collisions
• Increased temperature allows more collisions to exceed the activation energy, accelerating the reaction


  True
• What is an example of a slow reaction mentioned in the material?

  Rusting of iron
• The rate of reaction is often expressed as the change in concentration of reactants or products per unit time
• What two conditions must be met for a collision to result in a reaction according to collision theory?

  Correct orientation and sufficient energy
• What type of collision results in no reaction?

  Ineffective collision
• Increased temperature leads to a faster reaction rate because more molecules have sufficient energy to overcome the activation energy barrier.


  True
• Why does increasing surface area increase reaction rate?

  More frequent collisions
• Catalysts are consumed during a reaction.

  False
• What is the rate of reaction expressed as?

  Change in concentration per time
• What are the two conditions that must be met for a collision to result in a reaction according to collision theory?

  Correct orientation and sufficient energy
• Why does increasing temperature speed up a reaction according to collision theory?

  More collisions overcome activation energy
• Match the type of collision with its characteristics:

  Effective collision ↔️ Correct orientation and sufficient energy

  Ineffective collision ↔️ Incorrect orientation or insufficient energy
• What is an example of a fast reaction mentioned in the material?

  Explosions
• What is an example of a slow reaction?

  Rusting of iron
• The rate of reaction measures how fast reactants are consumed and products are formed.

  True
• An effective collision requires sufficient energy to overcome the activation energy barrier.


  True
• How does temperature affect molecular kinetic energy?

  Higher temperature increases it
• Match the concentration level with its effect on reaction rate:

  Increased concentration ↔️ Faster reaction rate

  Decreased concentration ↔️ Slower reaction rate
• How do catalysts affect activation energy?

  Lower activation energy
• Fast reactions occur quickly, with reactants rapidly converting into products
• How does temperature affect the rate of reaction?

  1️⃣ Higher temperature increases molecular kinetic energy

  2️⃣ More frequent and energetic collisions occur

  3️⃣ Reaction rate increases
• What happens to the reaction rate when the concentration of reactants is decreased?

  It slows down
• The likelihood of successful reactions increases with more frequent collisions
• What is an example of a fast reaction?

  Explosions
• Match the reaction type with its rate of reaction:

  Fast reactions ↔️ Occur quickly

  Slow reactions ↔️ Occur slowly
• The minimum energy required to start a reaction is called activation energy.
• Higher concentration leads to more frequent collisions between reactant molecules.
• Finely dividing solid reactants increases their surface area to speed up the reaction.
• Give an example of how temperature affects reaction rate in everyday life.

  Heating a cooking pan