The statement given is FALSE. The position of equilibrium for a reversible reaction can vary based on how the equilibrium was achieved. Here's an explanation to support this:
1. **Definition of Equilibrium:** In a reversible reaction, equilibrium is reached when the rate of the forward reaction equals the rate of the reverse reaction. At equilibrium, the concentrations of reactants and products remain constant over time.
2. **Factors Affecting Equilibrium:** The position of equilibrium is influenced by factors such as temperature, pressure, and concentration. Changes in these factors can shift the equilibrium position either to the left (favoring the reactants) or to the right (favoring the products).
3. **Le Chatelier's Principle:** This principle states that when a system at equilibrium is subjected to a change in conditions, it will respond by shifting the equilibrium to counteract the change. For example, if you increase the concentration of a reactant, the equilibrium will shift to the right to use up the excess reactant.
4. **Consequence:** Therefore, how the equilibrium was achieved (e.g., by changing temperature, pressure, or concentration) can impact the position of equilibrium. If you disturb the equilibrium, it will readjust to maintain a new equilibrium position based on the changes made.
In conclusion, the position of equilibrium for a reversible reaction is not always the same, as it can be altered by external factors. This highlights the dynamic nature of chemical equilibria and the importance of understanding how changes can affect the equilibrium position.
