Chapter 9 & 10: Rates & Extent of Reaction

• What is the harbour process used for?

  It is the industrial production of ammonia from nitrogen and hydrogen.
• Why is the harbour process considered important?

  Because ammonia produced is used to make nitrogen-based fertilizers for food production.
• At what temperature is the harbour process conducted?

  450 degrees Celsius.
• What pressure is used in the harbour process?

  200 atmospheres.
• What role does the iron catalyst play in the harbour process?

  It facilitates the reaction between nitrogen and hydrogen to form ammonia.
• Why is nitrogen easy to acquire for the harbour process?

  Because 78% of the air is nitrogen.
• How is hydrogen obtained for the harbour process?

  It is made from hydrocarbons like methane.
• What type of reaction is the harbour process?


  It is an exothermic and reversible reaction.
• What happens to the ammonia produced in the harbour process?

  It is separated from unreacted nitrogen and hydrogen for recycling.
• How is ammonia separated from nitrogen and hydrogen?

  By cooling the mixture in a condenser, allowing ammonia to condense into liquid.
• What are the three main considerations for the conditions used in the harbour process?


  • Percentage yield
  • Rate of reaction
  • Practical considerations (like cost)
• Why is a temperature of 450 degrees Celsius chosen for the harbour process?

  It is a compromise between achieving a higher yield and a higher rate of reaction.
• What is the effect of temperature on the yield and rate of reaction in the harbour process?

  A lower temperature favors yield, while a higher temperature increases the rate of reaction.
• Why is high pressure used in the harbour process?

  To achieve a high percentage yield and a high rate of reaction.
• What are the limitations of increasing pressure in the harbour process?

  Cost and safety concerns associated with maintaining high pressure.
• What is the best pressure used in the harbour process?

  200 atmospheres.
• What are the factors that affect the rate of chemical reactions?

  Temperature, concentration or pressure, surface area, and the presence or absence of a catalyst
• What is the theory behind chemical reactions known as?

  Collision theory
• According to collision theory, what must happen for particles to react?

  Particles must collide with each other with sufficient energy
• What is the term for the minimum energy required for a reaction to occur?

  Activation energy
• What happens if particles collide with less energy than the activation energy?

  They will bounce apart without reacting
• What two main factors determine the rate of a chemical reaction?

  The amount of energy the particles have and the frequency of collisions
• How does an increase in temperature affect the rate of reaction?

  It increases the energy of particles, leading to more frequent and energetic collisions
• Why are concentration and pressure considered a single factor in reaction rates?

  Both refer to the number of particles per unit of volume
• What effect does increasing concentration or pressure have on the rate of reaction?

  It increases the frequency of collisions, thus increasing the rate of reaction
• How does surface area affect the rate of reaction?

  A higher surface area increases the frequency of collisions
• If you wanted to react magnesium with an acid, which form would provide the highest rate of reaction?

  Powdered magnesium
• What is the role of a catalyst in a chemical reaction?

  A catalyst speeds up a reaction without being consumed in the process
• How does a catalyst affect activation energy?

  A catalyst lowers the activation energy by providing an alternative reaction pathway
• What is a common source of catalysts?

  Transition metals like cobalt and nickel
• What are enzymes in the context of catalysts?

  Enzymes are catalysts made by living organisms
• What are the key factors affecting the rate of chemical reactions?

  • Temperature: Increases energy and collision frequency
  • Concentration: More particles per unit volume
  • Pressure: More particles in gases
  • Surface Area: Higher area increases collision frequency
  • Catalyst: Lowers activation energy, increases successful collisions
• What are reversible reactions characterized by?

  They are characterized by a double arrow indicating that reactions can proceed in both forward and backward directions.
• What does the term 'equilibrium' refer to in reversible reactions?

  Equilibrium refers to the state where the forward and backward reactions occur at the same rate, resulting in constant concentrations of reactants and products.
• What does a one-way reaction indicate?

  A one-way reaction indicates that reactants can only turn into products and cannot revert back.
• In a reversible reaction, what do the top and bottom arrows represent?

  The top arrow represents the forward reaction, while the bottom arrow represents the backward reaction.
• What happens to the rates of the forward and backward reactions over time?

  The forward reaction starts fast and slows down, while the backward reaction starts slow and speeds up until they reach the same rate at equilibrium.
• What does it mean when a reaction is at equilibrium?

  It means that the concentrations of reactants and products remain constant because the forward and backward reactions occur at the same rate.
• Can the concentrations of reactants and products be equal at equilibrium?

  No, the concentrations can be different; equilibrium can still be reached with varying amounts of reactants and products.
• What does it mean if the equilibrium lies to the right?

  It means there are more products than reactants at equilibrium.