Law Of Chemical Equilibrium And Equilibrium Constant

The equilibrium constant for a reaction can be calculated by manipulating the equilibrium constants of the given reactions. To determine the equilibrium constant for the reaction: we must first combine the given reactions in such a way that we arrive at the desired reaction. Let's proceed step by step: - Reaction (a) gives us the equilibrium constant for: - Reaction (b) gives us the equilibrium constant for: - Reaction (c) gives us the equilibrium constant for: To derive the desired reaction, we can: 1. Multiply Reaction (a) by 2 to get on the left side. 2. Multiply Reaction (b) by 2 to get on the right side. 3. Multiply Reaction (c) by 3 to get on the right side. Thus, the equilibrium constant for the new reaction is the product of the equilibrium constants of the individual reactions raised to the appropriate powers:

The balanced chemical equation for the formation of HI is: Given: - The equilibrium constant at 700 K. - The initial concentration of HI is mol. - We are to find the concentrations of and at equilibrium. Let the initial concentration of HI be mol, and let the concentrations of and be mol at equilibrium. The stoichiometric change during the reaction will be: Since 2 moles of HI are produced from 1 mole of each and , for the reaction: - The change in concentration of and is (since 1 mole of each is consumed). - The concentration of HI increases by . Thus, at equilibrium: - The concentration of = - The concentration of = - The concentration of HI = Using the equilibrium constant expression: Substituting the equilibrium concentrations: Simplifying: Taking the square root of both sides: Now solve for : Thus, the concentration of and at equilibrium is . Thus, the correct concentration of and is .