equilibrium constants

Homogeneous and heterogeneous equilibria: Why are only gases and aqueous concentrations used when calculating Kc?

bc pure liquids and solids don’t vary in concentration, therefore, it doesn’t affect the equilibrium

E.g. gases are all compressible → therefore, changes in pressure will affect the equilibrium position if the number of moles on the reactant side differs from the product side. change is pressure → no effect on the solid present in the vessel

What is the effect of the magnitude of Kc?

if Kc > 1 → products are favoured. The greater the Kc, the further to the right lies the equilibrium position, i.e more products

if Kc < 1 → reactants are favoured. The smaller the Kc, the further to the left lies the equilibrium position i.e more reactants

How does Kc affect the equilibrium position?

If Kc = >1, the equilibrium position lies on the product side. The greater the value, the further to the right. Large Kc means we have mostly products.

If Kc = <1, the equilibrium position lies on the reactant side. The smaller the value, the further to the left. Small Kc means we have mostly reactants.

What is the relationship between Qc and Kc and how does it determine the equilibrium position?

Qc = Kc at equilibrium

If Qc>Kc → the equilibrium lies on the product side

If Qc<Kc → the equilibrium lies on the reactant side

What is the Equilibrium constant equation?

How do you calculate Kc with concentration?

How do you calculate Kc with RICE values?

R - ratio

I - initial

C - change

E - equilibrium