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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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randomwolfe randomwolfe
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11 years ago
Use the following half-reactions to write three spontaneous reactions, calculate E°cell for each reaction, and rank the oxidizing and reducing agents for each reaction. (Type your answer using the format [NH4]+ for NH4+, [Mg]2+ for Mg2+, and CO2 for CO2. Don't specify physical states. Use the lowest possible coefficients.)

(1) Au+(aq) + e-  Au(s)   E° = 1.69 V

(2) N2O(g) + 2 H+(aq) + 2 e-  N2(g) + H2O(l)   E° = 1.77 V

(3) Cr3+(aq) + 3 e-  Cr(s)   E° = -0.74 V


(A)  _____ N2O(g) + _____  _____(aq) + _____Cr(s) ----> _____  _____(g) + ____ ____(l) + _____ _____(aq)

   E°cell = ____V

   oxidizing agents: ______ >______
   reducing agents: _______>______   

(B) ______ Au+ _____  _____(aq) + _____ _____(s) ---> _____ _____(s) + _____ _____(aq)

   E°cell= _____V

   oxidizing agents:_____>______  
   reducing agents:_____>______

(C)  _____ _____(g) + ____ ____(aq) + _____ _____Au(s) ---> _____ _____(g) + ___ _____(l) + ____ _____(aq)

   E°cell= _____V

   oxidizing agents: _____>_____ 
   reducing agents:_____>_____ 
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