Unit 1: Controlling the rate

Why is controlling the rate important in industrial processes

If they are too low a manufacturing process will not be economically viable

Too high and there is the risk of thermal explosion

what must be true for a successful collision to take place

The particles must collide with sufficient energy (greater than or equal to the activation energy)

but also the correct collision geometry- the reactant particles have to be facing the right way. This is so that the activated complex can be formed

What is activation energy?

The certain minimum kinetic energy particles must collide at to overcome the forces of repulsion between their electron clouds

What does activation energy act as

A barrier standing between the reactants and products

What does a reaction with a ‘very low barrier’ mean

It has a small activation energy and therefore the reaction will be fast and will occur spontaneously at room temperature

What does a reaction with a ‘high barrier’ mean

Extra energy must be supplied to the reactant particles to ensure that the energy of collision is greater than the activation energy

Formula for relative rate

1/time

Formula for time

1/relative rate

What does [Delta] H mean

Change in enthalpy