The voltaic cell described by the balanced chemical reactionhas a standard emf o

Question

The voltaic cell described by the balanced chemical reactionhas a standard emf of 0.35 V. Calculate the equilibrium constant(Kc) for the reaction at 298 K. Round your answer to 3significant figures.

2MnO42-(aq) + 2Hg2+(aq) 2MnO4-(aq) +Hg22+(aq) St. Red. Pot. (V) MnO4-/MnO42- +0.56 Hg2+/Hg22+ +0.91 Constants 0 °C = 273.15 K R = 8.314 J/(K x mol) Faraday's Constant 96485 C/mol The voltaic cell described by the balanced chemical reactionhas a standard emf of 0.35 V. Calculate the equilibrium constant(Kc) for the reaction at 298 K. Round your answer to 3significant figures.

2MnO42-(aq) + 2Hg2+(aq) 2MnO4-(aq) +Hg22+(aq) St. Red. Pot. (V) MnO4-/MnO42- +0.56 Hg2+/Hg22+ +0.91 Constants 0 °C = 273.15 K R = 8.314 J/(K x mol) Faraday's Constant 96485 C/mol St. Red. Pot. (V) MnO4-/MnO42- +0.56 Hg2+/Hg22+ +0.91 Constants 0 °C = 273.15 K R = 8.314 J/(K x mol) Faraday's Constant 96485 C/mol

Explanation / Answer

G =-nFEcell= -RT ln K nFEcell= RT ln K (3)(96485)(.35) =(8.314)(298) ln K k =e^[((3)(96485)(.35))/((8.314)(298))]

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