Predict the proper equilibrium constant expression for the following reaction...
Fe(OH)3(s) ----> Fe3+(aq) + 3 OH-(aq) Explain the reasoning behind your answer.
K=products/reactants=[Fe3+][3OH]^3
K=[fe3+][OH-]^3
To predict the proper equilibrium constant expression for the given reaction, we need to understand the concept of equilibrium and how it relates to concentrations of reactants and products.
In any chemical reaction, reactants are converted into products. At equilibrium, the rate of the forward reaction (reactant to product) is equal to the rate of the reverse reaction (product to reactant), resulting in a constant concentration of reactants and products.
The equilibrium constant expression (Keq) is a mathematical representation that relates the concentrations (or partial pressures) of reactants and products at equilibrium.
For the given reaction:
Fe(OH)3(s) ----> Fe3+(aq) + 3 OH-(aq)
The equilibrium constant expression can be written as:
Keq = [Fe3+(aq)] * [OH-(aq)]^3
The reasoning behind this expression is based on the stoichiometry of the reaction. According to the balanced equation, one mole of solid Fe(OH)3 reacts to form one mole of Fe3+ ions and 3 moles of OH- ions.
Therefore, the equilibrium constant expression is obtained by considering the molar concentrations of each species at equilibrium. In this case, we raise the concentrations of Fe3+ and OH- to the power of their stoichiometric coefficients in the balanced equation.
It's important to note that the Keq expression is written using the concentrations of the species in the reaction, rather than their activities (in the case of solutions) or pressures (in case of gases), as long as the reaction is taking place in an ideal or near-ideal condition.