Properties of the Equilibrium Constant
if the leading coefficient of a reaction is multiplied by a factor of this number
What is the leading coefficient
initial, change, equilibrium is the meaning for this acronym
What is ICE
What is the difference between a homogeneous and a heterogeneous equilibrium
In a homogeneous equilibrium, all species are in the same phase. In a heterogeneous equilibrium, species are in different phases
This states that changing the reaction conditions of a system at equilibrium can knock the system out of equilibrium
What is LeChatelier's principle
What is the relationship between Q and K at equilibrium?
Q=K
if Q>K, this will happen
The products will decrease or the reactants will increase untill Q = K
These tables are used to organize equilibrium calculations
What are ice tables
Q equals this in a chemical reaction
the ratio of product concentrations to reactant concentrations at any given moment during a reaction
When an equilibrium system is stressed, the system will shift to reduce the stress and do this
get to equilibrium
What is the relationship between Q and K when stressed?
Q!=K
if Q<K, this will happen
The products will increase or the reactants will decrease untill Q = K
Depending on K this, the equilibrium conditions can be predicted.
What are stoichiometric coefficients
What is the effect of removing a product from an equilibrium system?
the reaction shifts forward to replace the removed product
If the reactant increases, the denominator of K does this
what is increases
If product concentration increases or reactant concentration decreases then this happens to Q
Q>K
When a reaction is reversed, Kreverse = this
1/Kforward
An ICE table is used to keep track of different values and calculate these
What are equilibrium conditions
How does increasing pressure affect a gaseous equilibrium system
causes the equilibrium to shift toward the side with fewer moles of gas
If the reactant does this, the system shifts to form reactant and consume product in response to the stress.
What is decreases
If product concentration decreases or reactant concentration increases then this happens to Q
Q<K
This is how you get your total for K
Multiply all K values
If Q is larger than K, this must decrease to make Q=K
What is the numerator
What does adding an inert gas do to a sealed equilibrium system
an inert gas increases total pressure but does not change the partial pressures
If the system is diluted, all molarity values will do this
What is decrease
you can do this to justify the response of an equilibrium system when stressed?
compare Q to K