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WMDhamnekar
MHB
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Equilibrium concentrations refer to the concentrations of reactants and products at a point where the forward and reverse reactions are occurring at the same rate. This means that the concentrations of reactants and products remain constant over time, and the reaction is said to be in a state of equilibrium.
Equilibrium concentrations in a homogeneous system can be determined using the equilibrium constant (K). This constant is calculated by dividing the concentration of products by the concentration of reactants, with each concentration raised to the power of its respective stoichiometric coefficient in the balanced chemical equation.
The equilibrium concentrations in a homogeneous system can be affected by changes in temperature, pressure, and the concentrations of reactants and products. Le Chatelier's principle states that when a stress is applied to a system at equilibrium, the system will shift in a direction that reduces the stress and re-establishes equilibrium.
Equilibrium concentrations do not directly impact the rate of a chemical reaction. However, they do affect the position of the equilibrium and the amount of products formed at equilibrium. Higher equilibrium concentrations of products indicate a higher yield of products and a faster rate of reaction.
Yes, the equilibrium concentrations in a homogeneous system can be changed by altering the initial concentrations of reactants and products. Adding or removing reactants or products will shift the equilibrium in a direction that reduces the stress and re-establishes equilibrium. This can change the equilibrium concentrations of all species involved in the reaction.