Static and Dynamic, Open and Closed Flashcards
What is a reversible reaction?
a reaction that can proceed in both the forward and reverse direction at the same time
What will eventually happen to ALL reversible reactions?
they will reach equilibrium
What is equilibrium?
the point in a reversible reaction where there is no change in the concentration of products and reactants (where the RATE of the forward and reverse reactions are equal)
What are the two types of equilibrium?
static and dynamic
Which of the two types of equilibriums are reversible?
dynamic only
Which of the two types of equilibriums are irreversible?
static only
Reversible reactions can only reach equilibrium in what kind of system?
closed system
What is a dynamic equilibrium?
a state of equilibrium where the forward and reverse reactions are constantly and actively occurring at the same rate. There is the same amount of movement in both directions
What is a static equilibrium?
a state of equilibrium where there are NO forward or reverse reactions occurring at all. There is the same amount of nothing happening, forward and reversed at the same rate
Which of the two types of equilibriums shows no visible change at all?
both dynamic and static
What is the reason that a reversible reaction would not act dynamically?
because it is in an open system, and some of the reactants might have escaped
What is a closed system?
a system that does not allow any interaction with the environment (outwards or inwards). Matter (reactants and products) can not enter or leave but energy (like heat) can
What is an open system?
a system where reactants or products might be lost to the environment, so equilibrium can not be reached. Matter (the reactants and products) and energy (like heat) can come in and out
Why can’t equilibrium be reached in an open system?
(hint: gaseous products)
As gaseous products are made, they escape the system. This means they will not build up enough to trigger the reverse reaction
What are the two situations that can cause static equilibrium?
1) when all the reagents or limiting reagents have been consumed and converted into products
2) When the activation energy of a reaction is too large to overcome under a particular setting e.g. temperature or pressure is too low. The movement between molecules/particles is too slow to overcome this energy.
