The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 6.8500 mol of F2(g) (Molar Mass - 38.00 g/mol) forms. Round your answer to 3 significant figures.
2F-(aq) + Mn2+(aq) �¨ F2(g) + Mn(s)
How do we relate work with the equation for electrochemistry?
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Is volts x coulombs = Joules?
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