3.2.2 Reaction Rates Flashcards
What’s the collision theory
For reactions to occur, particles must collide with each other with enough energy to break the bonds in the reactants
Why are only a small % of collisions successful
As there’s an energy barrier to breaking bonds
What do particles need to over come the barrier and react on collision
Enough energy (activation energy , Ea)
What are activation energies like for different reactions
Different
Define activation energy, Ea
Minimum amount of energy needed for a reaction to occur
What type of reaction has the most activation energy
Endothermic
What is the rate of reaction
+ equation
Change in concentration per unit time
Rate of reaction = amount of product produced/time taken
How could u work out the total number from a distribution curve
The area under the curve
What does the Maxwell-Boltzmann energy distribution curve show
The distribution of energies of particles in a gas
On Maxwell-Boltzmann energy distribution curve how many particles are at zero energy
0
On the Maxwell-Boltzmann energy distribution curve where does the curve never actually reach
Why
The x axis
As there will always be particles of very high energy
On the Maxwell-Boltzmann energy distribution curve what’s the area under the curve equal to
The total number of particles
What does the peak on a Maxwell-Boltzmann energy distribution curve indicate
The most probable energy (modal value/most common)
On Maxwell-Boltzmann energy distribution curve where’s the activation energy
What does this show you
The shaded bit to the left
Shows the amount of particles that can only react on collision
If temperature is increased what happens to the Maxwell-Boltzmann curve
Peak shifts to the right (higher energy)
Lower in height
Broader
