Nature of Chemical Reactions/Equilibrium Flashcards
Open and closed systems
Open system
- can exchange matter and energy with the surroundings
Closed system
- can only exhange energy with their surroundings
Reversible and irreversible reactions
Reversible
- when products can be used to reform reactants
- reactions that can proceed in the forward and backwards direction
- can only occur in a closed system
Irreversible
- reactions that can only proceed in the forward direction
Equilibrium
- when the rate of production of products is = to rate of reformation of reactants in a reversible reaction
dynamic equilibrium
- when the forward/backward reactions are still occuring
When is equilibirum determiend in a concentration/time graph
- as the concentration of reactants decrease, concentration of products increase
- over time, concentration of both level off and become constant –> equilibrium
Why does concentration never = zero
- as more products produced, greater chance of reactants being re-formed
what can concentration/time graphs indicate
The rate of reaction
- the steeper the curve, the quicker the RoR / the more that is being made at the point in time
Position of equilibrium
- compares the concentration of products/reactants at equilibrium
- if PoE lies to the right –> the reaction favours the products
- if PoE lies to the left –> reaction favours the production of reactants