Equilibrium shift refers to the change in the concentrations of reactants and products in a chemical reaction as it progresses towards equilibrium. It can occur when there is a change in the conditions of the reaction, such as temperature, pressure, or concentration of reactants or products.
Adding gas B to an A+B system can cause an equilibrium shift by changing the concentrations of the reactants and products. This can be due to the increase in the overall pressure of the system, which can favor the side with fewer moles of gas according to Le Chatelier's principle. It can also cause a shift if gas B is a reactant or product in the equilibrium equation.
The equilibrium will shift towards the side with fewer moles of gas when adding gas B to an A+B system. This is because an increase in pressure favors the side with fewer moles of gas according to Le Chatelier's principle. However, the exact direction of the shift also depends on the stoichiometry of the reaction and the equilibrium constant.
The concentration of gas B can affect the equilibrium shift in an A+B system depending on its role in the equilibrium equation. If gas B is a reactant, an increase in its concentration will shift the equilibrium towards the products, and vice versa. However, if gas B is a product, an increase in its concentration will shift the equilibrium towards the reactants.
Yes, the equilibrium can shift back to its original position after adding gas B to an A+B system. This can happen if the change in conditions is reversible, such as a change in pressure or concentration. The equilibrium will shift back until it reaches a new equilibrium point, where the rates of the forward and reverse reactions are equal again.