rate and extent of cc

• What does the rate of reaction tell us?

  It tells us how quickly reactants can be converted into products.
• Why is the fastest reaction not always the best in industry?

  Because maximum profit reactions prioritize cost over the rate of reaction.
• What is the trade-off in reaction rates in industrial processes?

  The trade-off is between speed, cost, and safety.
• How can you calculate the rate of reaction?

  By calculating the tangent's gradient.
• What does collision theory explain?

  It explains how reactions happen and why they occur at different rates.
• What is the minimum energy required for particles to react called?

  Activation energy.
• How can the rate of reaction be increased according to collision theory?

  By increasing the collisions or the energy of reacting particles.
• What are the five main factors that affect the rate of reaction?

  • Catalysts
  • Concentration of dissolved reactants
  • Pressure of gaseous reactants
  • Surface area
  • Temperature
• How do catalysts affect activation energy?

  Catalysts decrease activation energy and are not used up in the reaction.
• What is a key characteristic of catalysts in chemical reactions?

  They find alternative reaction pathways to lower activation energy.
• Why do catalysts need cleaning or regenerating?

  Because they can have environmental downsides in energy and waste.
• What are some examples of catalysts used in industry?

  Iron in the Haber process, platinum and palladium in catalytic converters, and enzymes in biological reactions.
• Why are catalysts typically in powder form?

  Because powders have the highest surface area for reactions.
• What are the advantages and disadvantages of using catalysts in industry?

  Advantages:

  • Cost-effective
  • Reduces combustion of fossil fuels

  
  

  Disadvantages:

  • Toxic to the environment
  • Hard to dispose of and can contaminate
• What are reversible reactions?

  Reactions where the products can reform the reactants.
• What does the equation A + B ⇌ C + D represent?

  It represents a reversible reaction where A and B react to form C and D, and C and D can react to reform A and B.
• What is the relationship between exothermic and endothermic reactions in reversible reactions?

  If the forward reaction is exothermic, the backward one will be endothermic.
• What does the conservation of energy state in reversible reactions?

  The energy absorbed/released by the forward reaction will equal the amount of energy released/absorbed by the backward reaction.
• What is dynamic equilibrium?

  Dynamic equilibrium occurs when the rates of the forward and backward reactions are equal.
• What does the term 'dynamic' imply in dynamic equilibrium?

  It implies that both the forward and backward reactions happen simultaneously.
• What happens to the concentrations of reactants and products at dynamic equilibrium?

  The concentrations of the reactants and products do not change at dynamic equilibrium.
• What defines a closed system in the context of equilibrium?

  A closed system is one where neither the products nor reactants can be added or removed, with no external factors acting on the reaction.
• How do changing conditions affect equilibrium?

  Changing conditions alters the amounts of products and reactants at equilibrium, affecting the position of the equilibrium.
• What is Le Chatelier’s principle?

  Le Chatelier’s principle states that a closed system at dynamic equilibrium will counteract any change applied to it.
• What factors can change the equilibrium position?

  • Temperature
  • Pressure (only affects gaseous reactions)
  • Concentration
• What happens to the equilibrium position when temperature is increased?

  An increase in temperature favors the endothermic reaction, increasing endothermic products and decreasing exothermic products.
• What occurs when the temperature is decreased in a reaction at equilibrium?

  A decrease in temperature favors the exothermic reaction, increasing exothermic products and decreasing endothermic products.
• How does an increase in pressure affect gaseous reactions at equilibrium?

  An increase in pressure favors the reaction that produces fewer gas molecules to reduce pressure.
• What is the Haber process used for?


  Making ammonia for ammonium fertilizers
• Why is the Haber process considered one of the world's most important reactions?


  It helps reintroduce nitrogen into the soil
• What is the balanced chemical equation for the Haber process?


  N2(g) + 3H2(g) ⇌ 2NH3(g)
• What is the enthalpy change for the forward reaction in the Haber process?


  • -92 kJ/mol
• What is the enthalpy change for the backward reaction in the Haber process?


  +92 kJ/mol
• What pressure is used in the Haber process, and why?


  200 ATM pressure favors the production of ammonia
• What temperature is maintained in the Haber process, and what is its effect?


  450 °C provides enough kinetic energy but favors the backward reaction
• What type of catalyst is used in the Haber process?


  Iron catalyst
• What happens to N2 and H2 in the Haber process?


  • Compressed
  • Heated
  • Condensed
  • Reused
  • Liquid ammonia leaves the reaction basin