Rates of reactions, catlysts boltzman Flashcards
definition of rate
The change n concentration of a given reactant/ product in a given time
Why doesn’t it matter whether reactants or products rates are measured
THEY BOTH MIRROR EACH OTHER, SO WE MEASURE THE EASIER ONE
What is the collision theory
In order for a chemical reaction to occur
reactant species must:
COLLIDE
POSSESS Ea
Macromolecules must be CORRECTLY ORIENTATED
wHAT FACTORS AFFECT RATE AND HOW
TEMPERATURE
CONCENTRATION > PROB OF SUCCESSFUL COLLISIONS
PRESSURE
SURFACE AREA
CATALYST
INCIDENT RADIATION
hOW does increasing concentration. icnrease rate
increase number of particles in a given volume
closer together- > chance of successful collisions
> frequent collision
> collide with greater energy than Ea
effect of increasing pressure on rate
Same number of molecules occupey a SMALLER VOLUME
CLOSER TOGETHER
> CHANCE PF COLLISIONS
>FREQUENT COLLISIONS
>COLLISIONS WITH ENERGY GREATER THAN ACTIVITY ENERGY
DEFINITION OF BOLTZMANN DISTRUBUTION
The distrubution of energies of molecules
at particular temperatures
often shown as a graph
WHy is the graph not symmetrical
Mass of each molecule is the same, but not the energy they possess
How does a graph with increased temperature differr from a normal graoh and why
At higher temperature the molecules have > Ke
distrubution flattens, shifts to the right
number of molecules in system doesn’t change
Molecules in the region of Ea increases
