1 Chemical Equilibrium Flashcards
(10 cards)
Do reactions always finish?
Reactions do not always finish. Some reactions find a balance between reactants and products.
What are the conditions required for an equilibrium?
Equilibriums only form in a closed system.
Differentiate between open and closed system.
Open system exchanges heat and matter with the environment. Closed system can only exchange heat.
What type of reactions are usually reversible?
Physical changes are usually reversible, whereas only some chemical reactions are reversible.
What are reactions that always finish called?
Complete reactions, irreversible reactions.
What are reactions that find a balance called?
Reversible reactions.
Explain approaching equilibrium at an atomic and molecular level.
Molecules of N204 are decomposing to form NO2, faster than molecules of No2 are reacting to form n2o4. We can see the gas getting darker as more no2 is formed.
Explain at equilibrium at an atomic and molecular level.
Molecules of n2o4 are decomposing as quickly as molecules of no2 are reacting (reaction is still occurring equally). Hence, concentrations of these gases do not change, and the colour of the gas does not change.
Define dynamic equilibrium.
A process that occurs in a closed system with a reversible reaction. It is called dynamic as reactions still occur, but are not visible/measurable. Dynamic equilibrium responds/opposes change.
Explain the direction of reactions according to collision theory.
- Reactant conc high, more collisions occur, RR high
- As reactant molecules are used, less collisions, RR slows
- As product conc increases, their collisions will be more prevalent and the rate of reverse reaction increases
- Eventually, the rate of the forward reaction and reverse reaction will be equivalent
!! Rate does not equal extent !!
