C5 - Kinetics Flashcards
What is activation energy
The minimum amount of energy that colliding particles must have for a successful collision leading to a chemical reaction.
Why do most collisions not lead to a reaction
The colliding particles don’t have energy to overcome the activation energy barrier
They may also be orientates incorrectly
Y axis of a Maxwell Boltzmann distribution curve
Number of particles with energy
X axis of a Maxwell Boltzmann distribution curve
Energy
Temperature increases rate of reaction because
Increased kinetic energy, so more frequent collisions
And higher proportion of collisions with energy greater than the activation energy.
How does Increased concentration increase rate of reaction
More particles in a given volume so more frequent collisions
How does pressure increase rate of reaction for gasses
The particles are more compressed so their concentration is higher, therefore increasing collision frequency
What is a catalyst
A substance that increases rate of reaction without being changed chemically or physically
How do catalysts work
They provide an alternative reaction route with lower activation energy
