3.1.5 Kinetics Flashcards
What is the definition of successful collisions?
When particles hit into each other and react as particles that have energy greater than or equal to the activation energy.
What is activation energy?
The minimum energy required for a reaction to occur.
What is a catalyst?
A chemical that lowers the activation energy by providing an alternate reaction pathway without being used up.
What are the effects of temperature on a reaction?
As the temperature increases/decreases the number of particles with energy equal to or greater than the activation energy increases/decreases. Which greatly increases/decreases the number of successful collisions.
What are the effects of pressure, surface area and concentration on a reaction?
The number of collisions will increase/decrease so the number of successful collisions with the required activation energy increases/decreases.
What are the effects of a catalyst on a reaction?
The proportion of particles with energy equal to or greater than the activation energy increases so the number of successful collisions increases.
