->> - At 355 K, AG = -5.7 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are 6.65 atm and 0.110 atm respectively, what is the standard free energy for this reaction at this temperature?

Delta H degrees and Delta S degrees for a reaction are –11.7 kJ/mol and –105 J/mol K, respectively. At what temperatures (in K) will this reaction be spontaneous under standard conditions?

33. Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. MnO2 (s) ⟶ Mn(s) + O2 (g) H2 (g) + Br2 (l) ⟶ 2HBr(g) Cu(s) + S(g) ⟶ CuS(s) 2LiOH(s) + CO2 (g) ⟶ Li2CO3 (s) + H2O(g) CH4 (g) + O2 (g) ⟶ C(s, graphite) + 2H2O(g) CS2 (g) + 3Cl2 (g) ⟶ CCl4(g) + S2Cl2 (g)

At 725 K, AG° = -21.6 kJ/mol for the reaction A (g) + 2 B (g) - 3 C (g). If the partial pressures of A, B, and C are 0.420 atm, 0.110 atm, and 7.20 atm respectively, what is the free energy for this reaction?

Save this response. Question 21 The standard free energy for the reaction H2(g) + 12(s) +→ 2HI(g) is 2.60 kļ/mol at 25°C. Find Kp for the reaction at this temperature. R = 8.314 x 103 k]/K•mole (T = temp in K) O 7.0 O 7100 O 1.0 O 2.4 O 0.35 A Moving to another question will save this response. MacBook Pro SC F4 F5 F6 F7 F1 F2 F3 %23 24 & 2 3 4 5 6

At 1120 K, AG° = 89.1 kJ/mol for the reaction 3 A (g) + B (g) →2 C (g). If the partial pressures of A, B, and C are 11.5 atm, 8.60 atm, and 0.510 atm respectively, what is the free energy for this reaction? %3D

A certain reaction is spontaneous at 65 ° C. If the enthalpy change for the reaction is  15 kJ/mol,  what is the minimum value of  Δ S (in J/K · mol) for the reaction.

A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ

At 560 K, AG° = -26.5 kJ/mol for the reaction A (g) + 2B (g) → 3 C (g). If the partial pressures of A, B, and C are 0.420 atm, 0.110 atm, and 7.20 atm respectively, what is the free energy for this reaction?

The standard reaction free energy AGO= == -910. kJ for this reaction: 6 C(s) + 6H₂(g) + 3O₂(g) →C6H12O6(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. AGⓇ reaction x10 1 C₂H₁2O6 (s) → 2C (s) + 2H₂ (g) + O₂ (g) kJ 3 C6H₁2O6 (s). 6C (s) + 6H₂(g) + 30₂ (g) kJ 12 3 1 3C (s) + 3H₂(g) + - 12/0₂ (8) → — C₂H₁2 06 (8) kJ 6 12 X ?