Kinetics Flashcards
What is collision theory?
The concept that atoms may come into contact with each other and react in a successful collision
Explain activation energy
The min. amount of energy required for substances to react and produce products
How do collisions affect the rate of reaction?
The more successful collisions that happen, the higher the RoR and the more product produced in a certain time
Explain how temperature affects rate of reaction?
- particles have more KE,
- this means more particles have the required Ea,
- So the frequency and success of collisions increases
Explain how pressure/concentration affects rate of reaction?
- More gas particles in a volume,
- Increases the frequency of collisions,
- But not the success of collisions bc the KE has not been affected
Explain how surface area affects the rate of reaction?
How are the axis of a Maxwell-Boltzmann distribution curve labelled?
- x-axis is labelled as ENERGY
- y-axis is labelled as THE NO. OF PARTICLES
What are the features of a Maxwell-Boltzmann distribution curve that must be considered (2)?
- The curve starts at the origin because every particle has some kinetic energy
- The curve does not touch the x axis at the end
- The curve is skewed to the left
What does the peak of the Maxwell-Boltzmann distribution curve show and how is this labelled?
Shows the most probable energy of particles, labelled as Emp
Where is the mean energy plotted on a Maxwell-Boltzmann distribution curve?
Slightly right to the Emp
What does the area under a Maxwell Boltzmann distribution curve show?
It shows the number of particles
What is the definition of rate of reaction?
The amount of product formed in a specified time period
