3(b) Rates of reaction

Question 1

factors affecting rates of reaction?

Answer 1

• concentration of the reactant in solution
• temperature at which the reaction is being carried out
• surface area of solid reactant
• the use of a catalyst

Question 2

how does the use of a catalyst speed up a reaction?

Answer 2

it lowers the activation energy as it creates an alternative pathway requiring. This means that more particles will have enough energy to react when they come together.

Question 3

why does increasing factors increase the rate of reactions?

Answer 3

they increase the number of successful collisions which means that a greater portion of reactant particles collide to form product molecules.

Question 4

explain using collision theory why increasing he concentration of solution increases RoR:

Answer 4

• there will be more reactant particles in a given volume, allowing more frequent and successful collisions per second

Question 5

explain using collision theory why increasing he temperature of solution increases RoR:

Answer 5

• the particles will have more kinetic energy than the required activation energy, therefore there will be more frequent and successful collisions per second

Question 6

explain using collision theory why increasing he SA of a solid increases RoR:

Answer 6

• more SA of the particles will be exposed to the other reactant, producing a higher number of collisions per second