CHEM CHEM SLAY CHEM

• What must happen for a reaction to occur?

  Reacting particles must successfully collide
• What defines a successful reaction?

  A reaction that leads to products forming
• What is activation energy?

  Minimum energy for a reaction to occur
• How does increasing the rate of reaction affect collisions?

  It increases the chance of successful collisions
• What are the four ways to change the rate of a reaction?

  • Temperature
  • Concentration
  • Surface area
  • Catalyst
• What happens to particles at higher temperatures?

  Particles move faster and have more energy
• How does increasing temperature affect the rate of reaction?

  It increases the rate due to faster collisions
• What effect does increasing concentration have on reacting particles?

  It increases the number of reacting particles
• How does surface area affect the rate of reaction?

  Larger surface area increases collision chances
• What is a catalyst?

  A substance that speeds up a reaction
• How does a catalyst affect activation energy?

  It lowers the activation energy required
• What are the methods to measure the rate of reaction?

  1. Change in mass
  2. Volume of gas formed
  3. Formation of a precipitate
• How is the rate of reaction measured by change in mass?

  By recording mass loss as gas escapes
• What does a gas syringe measure during a reaction?

  The volume of gas produced over time
• How is the formation of a precipitate measured?

  By recording decrease in light intensity
• What is the definition of the rate of reaction?

  The speed at which a reaction occurs
• What happens to particles at higher pressure?

  More particles are in the same space
• How does higher pressure affect the rate of reaction?

  It increases the chance of successful collisions
• What defines a successful collision?

  A collision that leads to a reaction
• How does kinetic energy relate to temperature?

  Higher temperature means higher kinetic energy
• Why is surface area important in reactions?

  It increases the chance of successful collisions
• What is the role of a catalyst in a reaction?

  It speeds up the reaction without being consumed
• Why is measuring the rate of reaction significant?

  It helps understand reaction dynamics and efficiency
• How does pressure affect the rate of reaction?

  Higher pressure increases collision frequency