19.3 Controlling the position of equilibrium

Created by

Jayden Clauer

Cards (13)

The larger the value of Kc the further the equilibrium position to the right
The smaller the value of Kc the further the equilibrium position to the left
The numerical value of equilibrium constants can be changed by only altering the temperature
The value of an equilibrium constant is not affected by changes in concentration, pressure or the presence of a catalyst
In an exothermic reaction, the equilibrium constant decreases with increasing temperature
equilibrium position shifts to the left
equilibrium yield of products decreases
In an endothermic reaction, the equilibrium constant increases with increasing temperature
equilibrium shifts to the right
equilibrium yield of products increases
At equilibrium, Kc = [products]/[reactants]
change in conditions may move the system out of equilibrium
Ratio is no longer equal to Kc
Position of equilibrium shifts to restore Kc
In an endothermic reaction, an increase in temperature increases Kc
ratio increases to reach a larger value of Kc
products increase and reactants decrease
position of equilibrium shifts to the right
In an exothermic reaction, an increase in temperature decreases Kc
ratio decreases to reach a smaller value of Kc
products decrease and reactants increase
position of equilibrium shifts to the left
When the concentration of a reactant is increased
the ratio decreases
reactants decrease and products increase to restore Kc
position of equilibrium shifts to the right
If the concentration of a product is increased
ratio increases
reactants increase and products decrease to restore Kc
position of equilibrium shifts to the left
Pressure has a similar effect to changes in concentration
if pressure increases, side with more gaseous molecules increases more than the side with less gaseous molecules
ratio adjusts to restore the value of Kc
position of equilibrium shifts to the side with fewer gaseous molecules
A catalyst has no effect on the value of an equilibrium constant