What is K for the following reaction at 298K? O2(g) + 4H*(aq) + 2Fe(s) → 2FE2+(aq) + 2H2O(1) E°cell = 1.57 V AG° = -NFE°. cell =-RT In(K) R = 8.314 J/mol K F = 96,485 C/mol e Report your answer in the form 1.23E45 with 3 significant figures.

@ た曲8 [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following reaction at 298 K. Cr³+ (aq) + Fe2+ (aq) → Cr²+ (aq) + Fe³+ (aq) Which of the following statements are correct? Choose all that apply. On =1 mol electrons OK>1 U The reaction is reactant-favored. OAG° <0 cell

What is the spontaneity of the chemical system? Cu(s) + H+(aq) -> Cu2+(aq, 1M) + H2(g) standard state

Calculate AG° for the reaction shown below using the provided thermodynamic properties information. H2O2 (1) → 2 H2O () + O2 (g) Substance AH°; (kJ/mol) AS° (J/(mol•K)) H2O2 (1) - 187.8 232.9 H20 (1) -285.83 69.91 O2 (g) 205.0 -396.4 kJ/mol -350.5 kJ/mol -33.70 kJ/mol -1105 kJ/mol -417.2 kJ/mol

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Determine AG (in kJ) for the following reaction at 325 K when the concentrations of the species are as follows: NO₂= 10.00 M, N₂O4 = 14.3 M. AG°f (NO₂) = 51 kJ/mol, AG (N₂O4) = 97.7 kJ/mol. 2 NO2(8) N₂O4(8)

Calculate AG° and K, at 25 °C for the reaction 2 CO(g) + O2(g)→2 CO2(g) Is the reaction product-favored or reactant-favored under standard conditions? Thermodynamic Data: G'r (kJ/mol) Species CO(g) CO2(g) -137.17 -394.36 AG° = kJ/mol K, = O product-favored O reactant-favored

What is the value of the equilibrium constant for the following reaction at 25C with a delta Grxn = -6.38 kJ?  H2(g) + Cl2(g) <-> 2HCl(g)

Calculate AH° for the following reaction 3 Fe203(s) + CO(g) – 2 Fez04(s) + C02(8). Species |AH°F, kJ/mol Fe2O3 (s) -824.2 Fe3O4 (s) -11184 CO (g) CO2 (g) -110.5 -393.5 O -577.2 kJ O- 723.3 KJ O -5213.4 kJ O -47.2 kJ