Final answer:
The equilibrium constant (K) for the reaction of maltose with H₂O₂ producing glucose is calculated using the concentration of glucose, which is 0.2 M. As the reaction is presented, we do not include H₂O₂ in the equilibrium expression because it is a liquid in its standard state. Therefore, K is 0.2 M under the given conditions.
Step-by-step explanation:
To calculate the equilibrium constant (K) under standard transformed conditions for the reaction of maltose with H₂O₂ producing glucose, we need to use the reaction quotient (Q) formula, since the equilibrium concentrations are given, rather than the standard state concentrations. The general reaction can be written as: maltose + H₂O₂ → glucose. However, since the exact reaction is not completely defined here (e.g., stoichiometry, phases), we'll assume that the coefficients of maltose and glucose are both 1, as often is the case in simple transformations, and that H₂O₂, being a liquid in its standard state, does not appear in the equilibrium expression.
Given:
Concentration of H₂O₂, [H₂O₂] = 0.5 M
Concentration of glucose, [glucose] = 0.2 M
The equilibrium constant expression (assuming the reaction proceeds as follows: maltose + H₂O₂ → glucose) for the reaction is K = [glucose]. Since the concentration of pure liquids and solids do not appear in the equilibrium expression, we only include the concentration of glucose in the K expression. Therefore, the equilibrium constant under the given conditions is simply K = [glucose] = 0.2 M.
It's also important to note that if the reaction involves more species with specific stoichiometry or if maltose were to remain in the equilibrium mixture, we would include those concentrations raised to the power of their stoichiometric coefficients in the expression for K. Additionally, the unit of the equilibrium constant depends on the reaction and would be dimensionless if the stoichiometry of products and reactants are the same. However, since the provided reaction is not balanced with stoichiometry, we include the Molarity (M) in the unit.
In summation, for the described reaction, the equilibrium constant (K) is 0.2 M under the given conditions.