Question

Manganese [Mn (I)] is soluble in water and is present in many groundwaters because insoluble forms (e.g, MnO) that are con- tained in minerals are reduced to soluble forms. The initial reactant concentrations are as follows: potassium permanganate (KMnO4), 8 mg/L; Mn2+,2 mg/L. Permanganate is sometimes used to remove Mnand the half reactions are MnoMnO E0.590 V Answer C, D, E please a. Balance the overall redox reaction. Which reaction is the oxi dation reaction Which is the reduction reaction? Identify the clectron acceptor and donor as well as the reductant and the oxidant. b. Calculate the cquilibrium constant. c. Calculate the equilbrium Mnconcentration when the pH is 7 and the concentration of potassium permanganate is I mg/L d. Obtain expressions for permanganate and Mno concentrations in terms of Mn + concentration e. Plot the frec energy as a function of the conversion of Mn from 0.01 to 0.999 Hint: Use the stoichiometric table to determine a reacting species as a function of Xa and then eliminate Xa by using the final concentration, Ca. After substituting Ca back into the expressions, the permanganate and MnO concentrations can be obtained in terms of the final concentration of Mn2

Answer 1