3.15 - kinetics & 3.16 - equilibrium Flashcards
What is the definition of activation energy?
The minimum energy required for reactant particles to collide and the reaction occurring
Why do not all reactions occur
- not enough activation energy
- reactants not in the right orientation
What is the effect of concentration and pressure on ROR?
- more particles in a given volume
- more frequent successful collisions
- ROR increases
What is the definition of a catalyst?
a substance that increases the rate of a chemical reaction without being changed in chemical composition or amount
How do catalysts work?
by providing an alternative reaction route of lower activation energy.
What are the conditions of an equilibrium ?
- rate of forward and backwards reactions are equal
- concentrations of reactants and products are not changing
What is Le Chatelier’s principle?
When a factor is changed an equilibrium will shift to oppose that change
How does a catalyst effect the yield of a reaction?
No effect
How does pressure effect yield?
Increased pressure = increased yield
How does temperature effect yield?
Increased temperature = decreased yield
Affect on Yield - pressure (model answer) 3 marks
- the yield increases/decreases
- because there are more/less moles on the left/right
- therefore equilibrium shifts to oppose the increase/decrease
Affect on Yield - temperature (model answer) 3 marks
- the yield increases/decreases
- because the forwards/backwards reaction is exo/endothermic
- therefore equilibrium shifts right/left to oppose the increase/decrease in temperature
How do you know if a reaction is exothermic or endothermic
Exothermic: forward enthalpy change is -
Endothermic: forward enthalpy change is +
How does pressure effect how the equilibrium shifts
DECREASE pressure:
Equilibrium will shift to side with LESS moles
INCREASE pressure:
Equilibrium will shift to side with MORE moles
What factors effect Kc and Kp
ONLY temperature not pressure or catalyst