Equilibrium (2) Flashcards
Qc > Kc
The system attains equilibrium by moving to the left, favouring reactants.
When Qc exceeds Kc, the concentration of products is higher than what the equilibrium would allow.
Qc < Kc
The system attains equilibrium by moving right, favouring products.
If Qc is less than Kc,the concentration of products is lower than what the equilibrium would favor.
Increasing reactant concentration/decreasing product concentration (effect on Kc, direction)
No effect on Kc, towards products
Decreasing reactant concentration/Increasing product concentration (Kc, direction)
No effect on Kc, towards reactants
Exothermic increasing temperature (Kc, direction)
Kc decreases, towards reactants
In response to the increased temperature, the system would favour the endothermic direction (that absorbs heat) to alleviate the excess heat. The reaction shifts towards the reactants (which typically absorb heat)
Exothermic decreasing temperature (Kc, direction)
Kc increases, towards products
The system will shift in the direction that generates more heat to compensate for the loss, which is the production of products.
Endothermic increasing temperature (Kc, direction)
Kc increases, towards products
In an endothermic reaction, heat is absorbed towards products. Therefore, the equilibrium shifts toward the direction that absorbs heat to keep up with the temperature increase.
Endothermic decreasing temperature (Kc, direction)
Kc decreases, towards reactants
The system seeks to regain the lost heat to compensate for the temperature decrease. The equilibrium shifts in the direction that generates heat, which is the reverse
More gaseous products, decreasing volume (Kc, direction)
No effect on Kc, towards reactants
More gaseous products, increasing volume (Kc, direction)
No effect on Kc, towards products
More gaseous reactants, decreasing volume( Kc, direction)
No effect on Kc, towards products
More gaseous reactants, increasing volume (Kc, direction)
No effect on Kc, towards reactants
