Kinetics Flashcards
What is the equation for the rate of reaction
Change in concentration
———————————-
Change in time
What is the definition of reaction rate
The change in concentration of a reactant or product with respect to time
What is the definition of activation energy
The minimum amount of energy for a reaction to occur
What is the definition of catalyst
A substance that increases the rate of a chemical reaction but does not get used up
State the basis of the collision theory
- Particles collide and react
- Not every collision = reaction as it needs activation energy
- Particles must be correctly orientated - inappropriate orientation = no reaction
What are the limitations of the collision theory
- Rates in solution– can’t accurately explain
2. Not all reactions are one step collision process
What happens to the Maxwell-Boltzmann distribution curve when the temperature is increased
Curve goes higher at the end
Right
Broader
Lower
What are the factors that affect the rate of reaction
Temperature
Concentration
Pressure
Catalyst
What effect does increasing temperature have on the rate of a reaction and why
Increases energy which increases the number of successful collisions which increases the number of successful collisions per unit time
What effect does increasing concentration have on the rate of a reaction
Increase leads to increase in particles per unit volume
Increase number if collisions
Increase number of successful collisions per unit time
What effect does increasing pressure have on the rate of reaction
Increase
Particles are closer together
Increased number of collisions
Increase number of successful collisions per unit time
What effect does a catalyst have on the rate of a reaction
Increase
Alternative pathway of lower activation energy
Increase number of successful collisions per unit time
Draw the effect of a catalyst on the activation energy on a Maxwell-Boltzmann distribution curve
See notes
