KINETICS Flashcards
what needs to happen for a reaction to occur
parrticles need to collide
how can we find the rate
amount of reactant used/ time
what is the activation energy
the minium amount of energy for a reaction to occur
what properties are needed for collisions to occur
need to have enough kinetic energy
what is thee peak in a Maxwell boltzman cureve
potable energy
where is the mena energy found
towards thee right of the most potable
why does the maxwell boltzman distribution curve start from 0,0
0 particles have 0 energy
what is on the x axis
energy
what is the area past the activation energy tell us
these particles have energy greater than the activation energy
what happens to the graph when you increase the temperature
curve moves to the right
why is the area past the activation energy greater when wee increse tthe temperature
more particles have energy greater than the activation energy
what happens to the curve when we decrease the temperature?
moves to the left
why does the area past the acttivation energy lower when we decrease the temperature
fewer particles have energy less than the activation energy
what is the effect of temperature on the rate of reaction
particles at high temps
have more kinetic energy
which causes more collison amongst them
what does a s mall increasse in temperature do to the rate of reaction
incresaes it
what happen swhen we increase the pressure on the rate of reaction?
particles more compact
more collisions
increase the rate of reaction
what happens when we increase the concentration on the rate of reaction
more particles within a set volume
further collisons
increases rate of reaction
what is a catalyst
increase the rate of reaction
by providing an alternative pathway
with a lower activation energy
what is the area past the activation energy like when wee add a catalyst
it is bigger `
