Chemistry- The Collision Theory

-In order to react, the particles must collide with each other. They must collide with sufficient energy and the correct orientation. The more frequently the particles collide, the greater the rate of the reaction. If the collision results in products being formed then the collision  is described as being “effective”. Any factor that increases the “effective collisions” will make the reaction go faster. 

Factors that affect the rate of a chemical reaction:

-Temperature

-Concentration

-Surface Area

-Catalyst 

RATE means how fast the reaction occurs.

The smaller the time taken the greater the rate of the reaction.

Temperature- An increase in the temperature of the reactant particles means that the reactant particles will have greater kinetic energy. This will result in more effective collisions per unit time (seconds) and a greater rate of reaction. 

Concentration-No. of particles. When the concentration of the reactant (acid) particles increases, there are more reactant particles. There will be more effective collisions per unit time (second) and hence a greater rate of the reaction.  

Surface area- a greater surface area allows more reactant particles to be exposed and available for collisions. This increases the number of collisions per unit time.

Catalyst- The catalyst is a chemical substance that will increase the rate of the reaction without itself being used in the process. Lowers the activation energy. 

Activation energy is the initial energy required for a reaction

to occur. It could be provided in the form of heat or kinetic

energy.