RATE OF REACTION AND COLLISION THEORY

the rate of reaction = how fast a reaction takes place. 

Very fast chemical reaction: an EXPLOSION

Fast chemical reaction: BURNING OF FUELS EG. METHANE/PETROL 

Slow chemical reaction: RUSTING

There are several factors that affect the rate of reaction including:

• TEMPERATURE
• SURFACE AREA OF A SOLID
• CONCENTRATION OF SOLUTION

'For a sufficient reaction to occur, particles must collide together with sufficient energy.'

This is called the ACTIVATION ENERGY.

If the partcles do not have Activation Energy needed, they will just bounce off eachother. 

So.....

If there are more successful collisions per unit, the rate of reaction will INCREASE! 

HIGHER TEMPERATURE OF REACTANTS --> FASTER RATE OF REACTION

EG. eggs can cook faster in boiling water than in warm water.

You can also COOL reactants to slow the process down. 

When the temperature is increased, the particles have a higher kinetic energy so move faster with more energy, and so the chances of a SUCCESSFUL COLLISION are higher. 

More particles have the Activation Energy.

concentration= a measure of how much solute is dissolved in a solvent.

higher concentration of solution = faster R.O.R

-More reactants are present

-Chance of successful collisions is much HIGHER. 

If the reaction involves solids then the rate of reaction can be affected by surface area. 

If the solid is broken up into small pieces more particles are available to react because they are at the surface so:

GREATER SURFACE AREA = FASTER R.O.R