The electrochemical cell described by the balanced chemicalequation has a standa

Question

The electrochemical cell described by the balanced chemicalequation has a standard emf (electromotive force) of4.05 V. Calculate the value (kJ) for theG° of the cell. Round your answer to 3 significantfigures.

F2(g) + Mn(s) 2F-(aq) +Mn2+(aq)
St. Red. Pot. (V) Mn2+/Mn -1.18 F2/F- +2.87 Faraday's Constant F = 96485 C The electrochemical cell described by the balanced chemicalequation has a standard emf (electromotive force) of4.05 V. Calculate the value (kJ) for theG° of the cell. Round your answer to 3 significantfigures.

F2(g) + Mn(s) 2F-(aq) +Mn2+(aq)
St. Red. Pot. (V) Mn2+/Mn -1.18 F2/F- +2.87 Faraday's Constant F = 96485 C St. Red. Pot. (V) Mn2+/Mn -1.18 F2/F- +2.87 Faraday's Constant F = 96485 C

Explanation / Answer

We hae The emf of the electrochemical cell = 4.05 V Since G = -nFE Where G is the free energy change and F is thefaraday's constant. Therefore                         G = -2*96485*4.05                               = - 781528.5 J                               = - 781.52 kJ

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