flashcards & answering structure

• 6 factors affecting rate of reaction

  use of catalyst

  concentration of acid/solution

  surface area of solid

  type of acid (monobasic/dibasic/tribasic)

  temperature of acid/solution

  pressure of gases
• collision theory

  reacting particles will need enough energy to effectively collide in order to react
• activation energy

  least amount of energy that colliding reacting particles must possess with react with each other
• explain how the concentration of a solution is able to affect the speed of reaction

  as the concentration increases, number of reacting particles packed per unit volume increases. frequency of effective collisions between reacting particles increases, rate of reaction increases, resulting in higher rate of formation of products
• explain how the temperature of acid is able to affect the speed of reaction

  as the temperature of acid/solution increases, reacting particles gain more kinetic energy and move faster. more particles possesses energy equals to or greater than the minimum activation energy needed for the reaction to proceed. frequency of effective collisions between reacting particles increases, rate of reaction increases, resulting in higher rate of formation of products
• explain how the particle size of solid is able to affect the speed of reaction

  as the particle size decreases, the surface area for reaction increases. frequency of effective collision between reacting particles increases, rate of reaction increases, resulting in a higher rate of formation of products
• explain how the pressure is able to affect the speed of reaction

  as the pressure increases, molecules of gases are packed closer together, allowing more reacting particles per unit volume. frequency of effective collisions between reacting particles increases, rate of reaction increases, resulting in higher rate of formation of products
• explain how the use of catalyst is able to affect the speed of reaction

  catalyst provides an alternative pathway for reaction to proceed by lowering activation energy. more particles possesses energy more than or equal to the minimum activation energy needed for reaction to proceed
• explain how the use of catalyst is able to affect the speed of reaction

  catalyst provides an alternative pathway for reaction to proceed by lowering activation energy. more particles possesses energy more than or equal to the minimum activation energy needed for reaction to proceed. frequency of effective collisions between reacting particles increases, rate of reaction increases, resulting in higher rate of formation of products
• explain, with reference of collision theory, the effect of changing the type of acid on the speed of reaction

  sulfuric acid is a dibasic acid which produces 2 moles of hydrogen ions when dissolved in water. hydrochloric acid is a monobasic acid which produces 1 moles of hydrogen ions when dissolved in water. sulfuric has double the number of moles of hydrogen ions present per unit volume. frequency of effective collisions between reacting particles increases, rate of reaction increases, higher rate of formation of products
• what happens when calcium carbonate reacts with hydrochloric acid?


  effervescence is observed, white powder will dissolve to form a colourless solution
• what is the colour of calcium carbonate in solid state

  white
• why does the reaction of hydrochloric acid and calcium carbonate stop?

  the calcium carbonate has completely reacted with hydrochloric acid
• what happens when calcium carbonate reacts with sulfuric acid?

  very strong effervescence will be observed at first but reaction will suddenly stop
• why does the reaction of sulfuric acid and calcium carbonate stop?


  calcium sulfate which is an insoluble salt forms a coating around calcium carbonate, preventing the hydrogen ions from reacting with more calcium carbonate