5.6.1.3 Collision Theory and Activation Energy Flashcards
1
Q
What does collision theory explain?
A
- how various factors affect rates of reactions
2
Q
What does collision theory say about chemical reactions occurring?
A
- can only occur when reacting particles collide with each other
- with sufficient energy
3
Q
What is activation energy?
A
- minimum amount of energy particles need to react
4
Q
What are the factors that when increased, can speed up the rate of a reaction?
A
- temperature
- concentration of reactants in solution
- pressure of reacting gases
- surface area of solid reactants
- catalyst
5
Q
Why does increasing temperature increase the rate of reaction?
A
- particles have more kinetic energy
- so more frequent, successful collisions
- more particles are moving faster and have activation energy
6
Q
Why does increasing concentration increase the rate of reaction?
A
- greater number of reactant particles in solution
- so more frequent, successful collisions
7
Q
Why does increasing the pressure of gases increase the rate of reaction?
A
- same number of particles in a smaller volume, so closer together
- so more frequent, successful collisions
8
Q
Why does increasing the surface area increase the rate of reaction?
A
- smaller pieces = larger surface area
- means more particles are on surface exposed to other reacting particles
- so more frequent, successful collisions
9
Q
What is the relationship between rate of reactions and concentration/pressure/surface area (graph)?
A
- directly proportional
- increasing one of the factors increases the rate of reaction
10
Q
What is the relationship between rate of reactions and temperature (graph)?
A
- not directly proportional
- small increase in temperature will have a big effect on rate of reaction
