factors effecting rate of reaction + collision theory

collision theory

for a chemical reaction to take place the particles need to collide with eachother with sufficient energy

rate of chemical reaction is

how fast reactants are used up OR how fast products are formed

concentration

if you increase the amount of particles in the same volume/space then your increasing frequent successful collisions as they are more likely to collide

temperature

increases particles internal energy they move faster and collide more frequently with more energy

surface area

increasing surface are to volume ration keeps same amount of volume but increases area the particles can collide on increasing frequent successful collisions

a catalyst is

a substance that speeds up a reaction without being used up or broken down or used up

how does a catalyst speed up reaction

it offers a alternative energy pathway with a lower activation energy

activation energy is

the minimum amount of energy needed for a chemical reaction to start

rate of reaction =

reactants used up OR products formed/ time

how to read rate of reaction off graphs

change in y/ change in x = gradient but also mean rate of reaction

tangent= precise rate at a point