Consider the following reaction:

The reaction mixture at initially contains and . At equilibrium, . What is the equilibrium constant for the reaction?

Consider a reaction mixture using the equation shown. At equilibrium the partial pressure of is and the partial pressure of is . What is the partial pressure of in this mixture if at ?

Considering the reaction shown, if the partial pressures of , , and are each, is the mixture at equilibrium? If not which direction will the reaction proceed to reach equilibrium if ?

In the laboratory of and of are reacted in a beaker. At equilibrium of remain. Using the equation shown calculate the equilibrium constant.

Find the of the reaction if you start with and end with at .

Determine the acid dissociation constant expression for the given reaction.

Consider the following reaction:

Give the expression for the equilibrium constant for this reaction.

Calculate the equilibrium constant at for the reaction by using free energies of formation.

Hypobromous acid will dissociate in water at with a . What is the for this dissociation process?