Kinetics Flashcards
(11 cards)
when can reactions occur
when particles collide with sufficient energy
activation energy definition
minimum energy with which particles need to collide in order for a reaction to be successful
what does the peak on m-w distribution curve represent
post probable energy
how many particles have enrgy above Ea
very few (far to right on m-w distribution curve)
why does energy on m-w distribution curve never meet the x axis
it is not possible for particles to have zero energy
how can a reaction go to completion if very few particles have energy over activation energy
particles gain energy through collisions
what does the maxwell boltzman curve look like at higher temperatures
curve shifts right, number of molecules with energy over Ea increases, number of particles with mp energy decreases
overall area under curve stays the same
particles have a wider range of energies
rate of reaction definition
change in concentration of substance in unit time
where is rate of reaction fastest
at the start (straighter part of graph)
effect of increasing pressure/ conc. on rate of reaction
faster as there are more particles per unit area so more frequent collisions. The relationship is directly proportional.
effect of using a catalyst on rate of reaction
A catalyst provides an alternative route with lower activation energy. So more collisions will be successful.
