T9 - Kinetics I Flashcards
1
Q
Rate of reaction
A
The change in concentration of a reactant or product per unit time
2
Q
Activation energy
A
The minimum energy needed for a successful collisions, leading to a reaction
3
Q
Collision theory -
What is needed for a reaction to take place
A
- Enough energy to meet the activation energy
- The correct orientation
4
Q
What are the 5 factors affecting rate of reaction
A
- Temperature
- Concentration
- Surface area
- Pressure
- Catalyst
5
Q
Why does increasing the temperature increase rate of reaction?
A
- Increases the average kinetic energy of all particles
- There are more frequent collisions and higher energy collisions
- There is now a greater proportion of collisions meeting the activation energy requirement
- More successful collisions
6
Q
Why does using a catalyst increase rate of reaction?
A
- Provide an alternate route for a reaction with a lower activation energy
- Usually orientate reactants favourably for a reaction to occur.
- More successful collisions
7
Q
Heterogeneous catalysts
A
Different phase to the reactants
8
Q
Homogeneous catalyst
A
Same phase as the reactants
9
Q
Why are transition metals such good catalysts?
A
Where reaction involve the transfer of electrons, transition metal are able to act as intermediates by varying their oxidation state
10
Q
A
