Chemistry – Rate of Reaction

Question 1

Rate of reaction

Answer 1

Definition: The rate of reaction is the speed at which reactants are converted into products.
Measured by the change in concentration of reactants or products over time.

Question 2

Fast vs slow reactions

Answer 2

Fast reactions: Occur in seconds or minutes, e.g., combustion or acid-base reactions.
Slow reactions: Take longer, from hours to years, e.g., rusting of iron or fermentation.

Question 3

The Collision Theory and the 3 conditions which need to be met for a reaction to occur

Answer 3

Collide with sufficient energy (activation energy).
Collide with correct orientation.
Collide with enough frequency.

Question 4

The different factors that can affect the rate of a reaction including temperature, concentration, agitation, surface area, and catalysts.

Answer 4

Temperature: Higher temperatures increase kinetic energy, leading to more frequent and energetic collisions.
Concentration: Higher concentration of reactants results in more particles in a given volume, increasing the frequency of collisions.
Agitation (stirring): Ensures particles are mixed, increasing the chances of collision.
Surface Area: Breaking solids into smaller pieces exposes more particles to react, increasing collision opportunities.
Catalysts: Catalysts lower activation energy, providing an alternative reaction pathway, which speeds up the reaction without being consumed.