To calculate the equilibrium constant Kc for the reaction, we first need to determine the concentrations of all species at equilibrium. The balanced equation for the reaction is:I2 aq + 2KI aq 2K+ aq + 2I- aq At equilibrium, the concentration of iodine I2 is given as 0.008 M, and the concentration of potassium iodide KI is given as 0.15 M. Since the stoichiometry of the reaction shows that 1 mole of I2 reacts with 2 moles of KI, we can determine the change in concentration for each species.Change in concentration of I2 = -0.008 M consumed Change in concentration of KI = -2 * 0.008 M = -0.016 M consumed Change in concentration of K+ = 2 * 0.008 M = 0.016 M produced Change in concentration of I- = 2 * 0.008 M = 0.016 M produced Now, we can determine the equilibrium concentrations of each species:[I2] = 0.008 M initial - 0.008 M change = 0 M[KI] = 0.15 M initial - 0.016 M change = 0.134 M[K+] = 0 M initial + 0.016 M change = 0.016 M[I-] = 0 M initial + 0.016 M change = 0.016 MNow we can calculate the equilibrium constant Kc using the expression:Kc = [K+]^2 * [I-]^2 / [I2] * [KI]^2 Plugging in the equilibrium concentrations:Kc = 0.016 ^2 * 0.016 ^2 / 0 * 0.134^2 Since the concentration of I2 is 0, the denominator becomes 0, and we cannot divide by 0. This indicates that the reaction has proceeded to completion, and there is no equilibrium between the reactants and products. In this case, we cannot calculate an equilibrium constant Kc for the reaction.