Rate of Reaction

particles must collide must have enough energy to react

• increase in concentration = increase in rate • increase in pressure = increase in rate because both result in more particles in a given volume so more collisions occur

• no molecules have zero energy • straight line flattens to peak • exponential curve

minimum energy needed for a collision to be successful and a reaction to take place (kjmol -1​)

at T1 - distribution shows how many particles have a minimum energy for activation energy at T2 - mean energy of particles increases (larger area shaded shows more particles have activation energy, more collisions successful so rate is faster

• substance that increases the rate of reaction without itself being used up by providing an alternate route for the reaction that has a lower activation energy • lower activation energy ensures that more particles will have it • more collisions successful, rate will increase

• homogenous catalyst • heterogenous catalyst

• catalyst and the reactants are both present in the same phase (e.g. both liquid) • catalyst and reactants present in different phases

change in concentration of reactants per unit time

delta[] / delta t

find tangent at that point

increase surface area = increase rate greater frequency of collisions more successful collisions per second

moldm-3s-1