Use the following half-reactions to write three spontaneous reactions, calculate

Question

Use the following half-reactions to write three spontaneous reactions, calculate E degree_cell for each reaction, and rank the oxidizing and reducing agents for each reaction. (Type your answer using the format [NH4] + for NH_4^+, [Mg]2 + for Mg_2^+, and CO2 for CO_2. Don't specify physical states. Use the lowest possible coefficients.) Au^+(aq) + e^- rightarrow Au(s) E degree = 1.69 V N_2O(g) + 2H^+ (aq) + 2e^- rightarrow N_2(g) + H_2O(I) E degree = 1.77 V Cr^3+(aq) + 3e^- rightarrow Cr(s) E degree = -0.74 V

Explanation / Answer

a) 3N2O(g) + 6H+(aq) + 2 Cr(s) ---------------------------> 3N2 (g) +3H2O(l) + 2Cr+3

b) E0cell= E0cathode- E0anode

         =1.77- (-0.74)

         = 2.51 V

c) 3N2O(g) + 6H+(aq) + 2 Cr(s) --------------------------->3N2 (g) +3H2O(l) + 2Cr+3

(OA)                                  ( Reduing Agent)                                (Reducing Agent)                             (Oxidizing Agent)

          oxidising agents : N2O > Cr^+3

         reducing agents     Cr > N2

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