Topic 4: Introduction to Kinetics Flashcards
Activation energy definition
The minimum energy required for a reaction to occur
Why do most collisions not lead to a reaction?
Reactants are not the correct orientation
They must have energy above the activation energy
Rate of reaction definition
Change in concentration of a reactant or product per unit time
Temp on rate of reaction
- More particles above kinetic energy
- Particles moving faster so more collisions
- More successful collisions per unit time
- Increased rate of reaction
Conc/ Pressure on the rate of reaction
Increased concerntration
More particles per unit volume
Increased frequency of collisions between reactants
More successful collisions per unit time
What is a catalyst
A substance that increases the rate of a reaction by providing an alternative reaction pathway with a lower activation energy.
Catalyst on rate of reaction
Provides an alternative reaction pathway with lower activation energy
More particles above activation energy
More sucessful collisions per unit time
Catalyst on rate of reaction
Provides an alternative reaction pathway with lower activation energy
More particles above activation energy
More sucessful collisions per unit time
What type of reaction is the dissapearing cross reaction
Precipitation reaction
