The Rate of Reaction examines how quickly reactants break down to form products.
Concept #1: Understanding Chemical Kinetics.
The word “kinetics” is derived from the Greek word “kinesis”, which means motion. So Chemical Kinetics deals with the speed of motion experienced by reactants as they are allowed to react.
Concept #2: Kinetics in a Chemical Reaction.
A chemical reaction is simply reactants breaking down and reassembling to form products.
Depending on certain conditions, a chemical reaction can either happen very quickly in seconds or take place over several years.
Concept #3: Slow vs. Fast Reactions.
Concept #4: Kinetics & the Concentration of Compounds.
In order for a chemical reaction to occur two molecules must collide. The more concentrated a solution then the greater the chance of them colliding.
Concept #5: Kinetics & the Surface Area of Compounds.
For a collision between molecules to be successful, molecules join at their active sites. The larger their surface area then the more places the molecules can successful join.
Concept #6: Kinetics & Temperature.
The General Rule is increasing the reaction temperature by 10oC will cause the rate to double.
Concept #7: Kinetics & the Catalyst.
A catalyst helps to speed up the rate of a reaction by lowering the energy of activation (Ea).