 | Term | Definition |
| |
Kinetics |
The speed at which reactions occur |
| |
Reaction Rates |
The change in concentration of reactants and products in a certain amount of time |
| |
Rate Law |
The concentration of the reactants to the rate of a reaction |
| |
Collision Theory |
Depends upon the collisions between reacting particles |
| |
Surface Area |
a larger surface area increases the frequency at which particles collide; when particles collide more often, there is a higher chance for effective collisions to take place |
| |
Concentration |
an incrase means that there are more particles within a given volume; smaller distances higher probability of collisions; more collisions within a given amount of time mean a faster reaction rate |
| |
Nature of Reactants |
the composition of reactants and complexity of the bonds that have to be broken and formed in order for the reaction to proceed affects the reaction rate |
| |
Temperature |
measure of teh average kinetic energy for the particles in a substance, increase usually increases the rate of reaction |
| |
The Rule of Thumb |
For each 10C increase in temperature, the reaction rate doubles |
| |
Presence of a catalyst |
substance that increases reaction rate without being consumed during reactions; change teh reaction mechanism by lowering the activation energy |
| |
Natural catalyst |
enzymes |
| |
Pressure |
Only affects the reaction rates of gases |
