rate of reaction

• What is the rate of reaction?

  How quickly reactants turn into products
• How is the rate of reaction calculated for reactants?

  Quantity of reactant used divided by time taken
• How is the rate of reaction calculated for products?

  Quantity of product formed divided by time taken
• What is required for a reaction to occur according to collision theory?

  Reactant particles must collide with enough energy
• What is the term for the minimum energy needed for a reaction?

  Activation energy
• How can the rate of a reaction be increased?

  • Increase frequency of collisions
  • Increase energy of particles during collisions
• How does increasing temperature affect the rate of reaction?

  Particles move faster, leading to more collisions
• What happens to particles when temperature is increased?

  Particles have more energy, causing more reactions
• How can the concentration of solutions be increased?

  Use a solution with more solute in the same solvent
• What effect does increasing concentration have on reaction rate?

  More reactant particles lead to more frequent collisions
• How can the pressure of gases be increased?

  Increase the number of gas particles or reduce container size
• What is the effect of increasing pressure on reaction rate?

  Less space between particles means more collisions
• How can the surface area of solids be increased?

  Cut solids into smaller pieces or grind them
• Why does increasing surface area affect reaction rate?

  More surface area exposes more reactant particles
• What are catalysts?

  Substances that increase the rate of reaction
• How do catalysts affect activation energy?

  Catalysts provide a pathway with lower activation energy
• What is the result of using a catalyst in a reaction?

  More particles collide with enough energy to react