TRUE or FALSE: The equilibrium constant of a reaction can change if the concentration of reactants and products are changed.
The correct answer and explanation is:
Answer: FALSE
The equilibrium constant (K) of a reaction is a fixed value at a given temperature, and it does not change when the concentrations of reactants or products are altered. This is because the equilibrium constant reflects the ratio of the concentrations of products to reactants, each raised to the power of their respective coefficients in the balanced chemical equation.
The equilibrium constant is a function of temperature, meaning it will change if the temperature of the system changes. However, changing the concentrations of reactants or products will only shift the position of equilibrium but will not affect the equilibrium constant itself. This is described by Le Chatelier’s Principle, which states that when a system at equilibrium is disturbed (for example, by changing the concentration of reactants or products), the system will adjust to counteract the disturbance and restore equilibrium.
For example, if more reactants are added, the equilibrium will shift towards the products to consume the excess reactants and reach a new equilibrium position. Similarly, if products are removed, the system will shift towards the products to replace the lost product. However, the ratio of the concentrations of products to reactants, as defined by the equilibrium constant, will remain unchanged unless the temperature is altered.
In summary, while changes in concentration can affect the concentrations of reactants and products at equilibrium, they do not change the equilibrium constant itself. Only temperature has the power to alter the value of the equilibrium constant.