)    Using a table of standard electrode potentials, predict whether the following reactions will be spontaneous, and calculate Eo for the reaction a)    Fe3+ (aq) + I- (aq) → Fe2+ (aq) + I2 (s) b)    Cl- (aq) + 2H2O → Cl2 (g) + H2 (g) + 2OH- (aq)

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8)    Using a table of standard electrode potentials, predict whether the following reactions will be spontaneous, and calculate Eo for the reaction

a)    Fe3+ (aq) + I- (aq) → Fe2+ (aq) + I2 (s)


b)    Cl- (aq) + 2H2O → Cl2 (g) + H2 (g) + 2OH- (aq)


c)    Ag (s) + H+(aq) + NO3-(aq) →  Ag+ (aq)

 

potential (V) reduction half- reaction
+2.87 F2(g) + 2 e- = 2F-(aq)
+1.33 Cr2 O7 2-(aq) + 14 H+(aq) + 6 e- = 2 Cr3+(aq) + 7 H2O(I)
+0.77 Fe3+(aq) + e- = Fe2+(aq)
+0.68 O2(g) + 2H+(aq) + 2 e- = H2O2(aq)
0 2 H+(aq) + 2 e- = H2(g)
-0.44 Fe2+ (aq) + 2 e- = Fe(s)
-0.83 2 H2O (I) + 2 e- = H2(g) + 2 OH-(aq)
-2.71 Na+ (aq) + e- = Na(s)
-3.05 Li+(aq) + e- = Li (s)

 

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