Question- The electrochemical cell described by the cell notation has a standard emf of 0.68 V. Calculate the maximum electrical work (kJ) the cell has done if 1.7200 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to three significant figures.
Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)
St. Red. Pot. (V)
VO2+/VO2+ +1.00
MnO4-/MnO2 +1.68
Faraday's Constant
F = 96485 C
Using textbook reference solve the reactions given in above problem