Given the following reduction half-reactions: Fe*(ag) + e → Fe2* (aq) Eed = +0.77 V S202- (ag) + 4 H*(aq) + 2 e → 2 H2SO3(aq) Ered = +0.60 V N20(8) + 2H*(aq) + 2 e¯ → N2(8) + H;0(I) Eed –1.77 V voj(aq) + 2H*(aq) + e- → VO2+ + H,0(I) Ered = +1.00V (a) Write balanced chemical equations for the oxidation of Fe2"(aq) by S20? (aq), by N20(aq), and by VO* (aq). (b) Calculate AG" for each reaction at 298 K. (c) Calculate the equilibrium constant K for each reaction at 298 K.

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGO for the following redox reaction. Round your answer to 3 significant digits. 2C1 (aq) + 2HNO₂ (aq) + 2H* (aq) → Cl₂ (g) + x10 +2NO(g) + 2H₂O (1) X

Both O2 +  2H2O +  4e− →  4OH−   and  O2(g) +  2H2O (I) →  4OH− (aq)

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Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. 4Br (aq) +N2 (g)+4H₂O (1) → 2Bг2 (1)+N₂H4 (aq) +40H (aq) OkJ T x10 ×

Write oxidation and reduction half reactions for the following: Fe2+(aq) + MnO4-(aq) → Fe3+(aq) + Mn2+(aq)

Examine the following half-reactions and select the strongest oxidizing agent among the substances. v Jersey Departm E° = 0.755 V [PtCl4]²¯(aq) + 2e¯ 2 Pt(s) + 4CI'(aq); RuO4(s) + 8H*(aq) + 8e¯ 2 Ru(s) + 4H2O(1); FeO4²(aq) + 8H*(aq) + 3e¯ 2 Fe3*(aq) + 4H2O(/); H4XEO6(aq) + 2H*(aq) + 2e¯ 2 XeO3(aq) + 3H2O(/); E° = 2.42 V E° = 1.038 V E° = 2.07 V RuO4(s) H4XEO6(aq) [PtCl4]² (aq) O HFEO4¯ (aq) CI(aq)

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy following redox reaction. Be sure your answer has the correct number of significant digits. H₂(g) + 2OH¯(aq) + 2Fe³+ (aq) → 2H₂O (1) + 2Fe²+ (aq) kJ x10 X Ś AGO for the

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