11: Equlibrium II
No description yet. This curated deck is ready for daily study.
Card preview (11)
What do we use Kp for?
Homogeneous gaseous equilibria - reactants and products use partial pressure instead of concentration so no square brackets
What is the expression for Kp?
The same as Kc but instead it’s partial pressure not concentration so you DO NOT USE SQUARE BRACKETS
What is the total pressure of a gaseous system at equilibrium directly related to?
The number of moles of each gas in the mixture
What is partial pressure?
How much pressure one type of gas contributed to the total pressure
How do you calculate partial pressure of a gas?
partial pressure of a gas = mole fraction of the gas x total pressure
What is the mole fraction of a gas?
The moles of that gas in the mixture compares to moles of all gases
How do you calculate the mole fraction of a gas?
Mole fraction of a gas = moles of a gas / total moles of all gases
What is the effect of increasing the temperate on Kp if the forward reaction is exothermic?
Shifts equilibrium to the left Kp decreases
What is the effect of increasing the temperate on Kp if the forward reaction is endothermic?
Equilibrium shifts to the right Kp will increase
What are the two conditions for dynamic equilibrium to be set?
1) The reaction must be reversible 2) The reaction mixture must be in a closed container
What are the three important features that define a system that is in dynamic equilibrium?
• Both forward and backward reactions are continuously occurring. • The rate of the forward reaction is equal to the rate of the backward reaction. • The concentration of products and reactants must be constant