Final answer:
When compound A is removed from the reaction A + B ⇌ AB, the equilibrium will shift in a direction to replace A, following Le Chatelier's Principle. An ICE table helps track changes in concentrations, and the reaction will continue until equilibrium is re-established and concentrations become constant.
Step-by-step explanation:
When compound A is removed from the equilibrium system represented by the reaction A + B ⇌ AB, the equilibrium will shift to counter the change by favoring the reaction that replaces compound A. This behavior is described by Le Chatelier's Principle, which predicts that a system at equilibrium will try to counteract any disturbance.
If we consider an initial scenario where 0.50 moles of A are added to a mixture at equilibrium, we have now 1.0 mol of A and 1.0 mol of B. An ICE table (Initial, Change, Equilibrium) is used to track changes in concentrations. During the shift toward equilibrium, the reaction quotient Qc changes and once equilibrium is reached again, concentrations of products and reactants remain constant.
Removal of A will cause the equilibrium to shift towards the left (the reverse reaction), increasing the concentration of A to replace what was removed. The reaction will continue to shift until the removed substance is replenished and equilibrium is re-established.