Final answer:
Equilibrium will shift to balance changes in system conditions according to Le Chatelier's principle, but without details on the number of moles on each side of the reaction, it's not possible to determine the direction of the shift when expanding the container.
Step-by-step explanation:
According to Le Chatelier's principle, changes in the condition of a system at equilibrium will result in a shift to counteract the change. If you expand the container of an equilibrium reaction, this effectively decreases the pressure. For a reaction with more moles of gas on one side than the other, the equilibrium will shift towards the side with more moles of gas to increase pressure. Conversely, if the reaction has fewer moles of gas on the side with products, decreasing the volume (or increasing pressure) will shift the equilibrium towards the products. However, the initial question you have provided does not specify the number of moles of reactants and products, therefore it is not possible to definitively state in which direction the equilibrium will shift without additional information.