Given the reaction A(g) + B(g) <-> 2AB(g)
1. What does equilibrium mean? -equal mols or pressure between reactants and products? Is there more reactants or products?
2. Will the equilibrium be the same if i started with the reactants only vs if i started with the product only. What are the similarities and differences between starting out with one or the other?
3. Once equilibrium is reach, will there be any changes to system 5 mins after equilibrium, 10 mins after equilibrium?
4. What is actually happening at the molecular level before and after equilibrium? Like do all collisions between A and B make AB? How does AB make A and B again?
1. Equilibrium is attained in a reaction when products are being formed at the same rate at which reactants are being formed; i.e., the forward reaction occurs at the same rate as the reverse reaction. Equilibrium is a dynamic process which means that the reaction still is taking place but there is no net change in the concns of reactants or products.
2. It makes no difference if you start with reactants or with products; at equilibrium, the concns of reactants and products will be the same no matter which you start with.
3. Forward and reverse reactions occur all the time; there is no NET CHANGE in the concns after equilibrium is attained.
4. Not all collisions between A and B produce AB but only those in which A molecules and B molecules have enough energy to produce a union. AB splits to make A and B.
1. Equilibrium refers to a state in a chemical reaction where the forward and backward reaction rates are equal. At equilibrium, the concentrations (or pressures in the case of gases) of the reactants and products remain constant. It does not necessarily mean that the molar amounts or pressures of the reactants and products are equal. The equilibrium position can vary depending on the relative concentrations of reactants and products.
2. Starting with the reactants only or starting with the products only will result in different equilibrium positions. If you start with only reactants, the reaction will proceed in the forward direction until equilibrium is reached. On the other hand, if you start with only products, the reaction will proceed in the reverse direction to form more reactants until equilibrium is established. The equilibrium concentrations will depend on the initial concentrations used, but the final equilibrium concentrations will be the same regardless of the starting materials.
3. Once equilibrium is reached, the concentrations of reactants and products will not change significantly over time, assuming no external influences or disturbances are introduced. Therefore, after the equilibrium is reached, the concentrations will remain constant, regardless of the time elapsed. In this case, 5 minutes, 10 minutes, or any other time after equilibrium is reached will not cause any changes to the system.
4. At the molecular level, before equilibrium is reached, collisions between molecules A and B can occur. However, not all collisions result in the formation of AB. Only certain collisions possess sufficient energy and proper orientation to lead to the formation of AB. This is known as the collision theory.
Once equilibrium is established, forward and reverse reactions are still occurring, but at equal rates. Some of the AB molecules can dissociate back into A and B, while some A and B molecules can collide to form more AB. At equilibrium, the rate of forward reaction is equal to the rate of reverse reaction, resulting in a dynamic balance where the concentrations of A, B, and AB remain constant.