Kinetics Flashcards
What is necessary for a reaction to take place
Collisions must take place between particles which have sufficient energy
What is the activation energy
the energy needed to ‘activate’ the reactant particles in order for them to collide effectively and cause a chemical reaction.
Why do most collisions not lead to a reaction
Molecules need to have a certain amount of kinetic energy and hit other molecules at the right orientation in order for the reaction to occur.
What do maxwell-boltzmann distributions tell us about energies
No particles have 0 energy
Most particles have intermediate energies
A few have very high energies
Average energy is not the same as most probable energy
How does increasing temperature effect a M-B distribution
The graph will be flatter
More particles with EA
Higher probable and average energy
How do catalysts work
They provide an alternate reaction path way
What is a catalyst
A substance that increases the rate of a chemical reaction without being changed in chemical composition or amount
How does a catalyst effect an M-B diagram
Decreases the EA needed
How does increasing reactant concentration effect rate of reaction?
Increasing the concentration of reactants increases the number of successful collisions between them and, as a result, the reaction rate
How does increasing reactant pressure effect rate of reaction?
If the pressure is higher, the chances of collision are greater.
Maxwell Boltzmann distribution graph
Maxwell Boltzmann distribution
Most probable energy is at peak
Average energy is to the right of the peak
