Physical 1: Kinetics

Question 1

what must particles do in order to react

Answer 1

collide with sufficient energy (activation energy) and the correct orientation

Question 2

do most collisions result in a reaction?

Answer 2

no

Question 3

define activation energy

Answer 3

the minimum energy that particles must collide with for a reaction to occur

Question 4

maxwell - boltzmann distribution

Answer 4

shows the number of molecules, most probable energy activation energy, and kinetic energy
* google a pic cuz i can’t add one in :) *

Question 5

what is the effect of increasing temperature on rate of reaction? why?

Answer 5

increasing temperature increases the rate of reaction
much higher proportion of particles have energy greater than the activation energy, many more successful collisions per second, increased rate

Question 6

what is the effect of increasing concentration/pressure on rate of reaction? why?

Answer 6

increased concentration/ pressure - increased rate of reaction
there are more particles in a given volume = more frequent successful collisions = increased rate

Question 7

what is a catalyst ?

Answer 7

a substance which increases the rate of reaction but is not used up in the reaction

Question 8

how to catalysts work and how do they increase the rate of reaction?

Answer 8

provide an alternative reaction pathway ( one with a lower activation energy )
lowers the activation energy, so more particles have energy greater than activation energy, so more frequent successful collisions, so increased reaction rate