Chapter 10 + 19 Flashcards
Reversible reaction
Can go in forward or backward direction
When does a reversible reaction reach dynamic equilibrium
When the rate of forward reaction = rate of backward reaction
Concentrations of the reactants and products
No further changes
Kc
Equilibrium constant in relation to concentration
Calculating Kc
[Product 1]^moles x [Product 2]^moles / [Reactant 1]^moles x [Reactant 2]^moles
When can equilibrium be reached
in a closed system (a system which can’t exchange matter or energy with the surroundings)
Le Chatelier’s Principle
The position of a dynamic equilibrium shifts to minimise the effect of the change
Reaction quotient
The concentration of the substances when the reaction is not at equilbrium
What is the reaction quotient at equilibrium equal to?
Equilibrium constant
Changing the temperature
- If the mixture is heated, it will favour the endothermic reaction
- If the mixture is cooled, it will favour the exothermic reaction
Changing the volume/pressure
Decreasing volume/increasing pressure:
Equilibrium shifts towards the side with less particles to lower the pressure and minimise the change
Increasing volume/decreasing pressure:
Equilibrium shifts towards the side with more particles to increase the pressure and minimise the change
How to calculate the partial pressure of any gas in a mixture
Moles/total moles x pressure
Adding reactant:
Effect: Shifts to right
Effect on K: no effect
Removing reactant
Effect: Shifts to left
Effect on K: no effect
Adding product
Effect: Shifts to left
Effect on K: no effect
