tsaitea said:The definition of stress (at least in my case) is a change in temperature, pressure or concentration in the system. For concentration we are talking about adding concentration to the system as a stress.
I was thinking maybe we can reduce the volume to shift the equilibrium concentrations downwards.
The equilibrium concentrations of a reaction can be determined by using the equilibrium constant (K) and the initial concentrations of the reactants and products. By setting up an ICE (initial, change, equilibrium) table and solving for the equilibrium concentrations, you can determine the concentrations at equilibrium without adding any stress.
Changes in temperature, pressure, or concentration of reactants or products can cause a shift in equilibrium concentrations. Additionally, changes in the volume of the container or the addition of a catalyst can also affect the equilibrium concentrations without adding any stress.
Le Chatelier's Principle states that when a stress is applied to a system at equilibrium, the system will shift in a direction that minimizes the effect of the stress. In the case of shifting equilibrium concentrations without adding stress, changes in temperature, pressure, or concentration can act as "pseudo-stresses," causing the system to shift in order to maintain equilibrium.
No, equilibrium concentrations are not affected by changes in the rate of the reaction. The rate of the reaction only determines how quickly the system will reach equilibrium, but it does not affect the final equilibrium concentrations.
The direction of the shift in equilibrium can be predicted by using the reaction's equilibrium constant (K) and the initial concentrations of the reactants and products. If the calculated Q value (reaction quotient) is greater than K, the reaction will shift towards the reactants. If Q is less than K, the reaction will shift towards the products. If Q is equal to K, the reaction is already at equilibrium and no shift will occur.