Given the reaction Cl2(g) + 2NO(g) → 2NOCl(g), if the standard Gibbs free energy change (ΔG°) for the reaction is negative, what can be concluded about the reaction at standard conditions?

At 1120 K, ΔG° = 78.9 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 Gibbs free energy change (ΔG) for this reaction under these conditions?

Calculate ΔG°rxn at 298 K for the following reaction: I2(g) + Cl2(g) ⇌ 2ICl(g), given that Kp = 81.9. Which of the following is the correct value of ΔG°rxn?

Calculate the Gibbs free energy change (ΔG_rxn) at 298 K for the reaction N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) given the standard Gibbs free energy change (ΔG° = -33.3 kJ) and the partial pressures: P(N2) = 1.5 atm, P(H2) = 4.5 atm, P(NH3) = 6.0 atm.

Calculate the Gibbs free energy change (ΔGᵣₓₙ) at 298 K for the reaction N₂ (g) + 3 H₂ (g) ⇌ 2 NH₃ (g) given the standard Gibbs free energy change (ΔG° = -33.3 kJ) and the partial pressures: P(N₂) = 1.5 atm, P(H₂) = 4.5 atm, P(NH₃) = 1.0 atm.

Determine the minimum pressure of N₂ required to keep the reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) spontaneous at 298 K, given ΔG°rxn = -33.3 kJ/mol, P H₂ = 1.00 x 10⁻² atm, and P NH₃ = 1.00 atm.

Estimate the value of the equilibrium constant at 660 K for the reaction 2NO2(g) ⇌ N2O4(g) given that ΔG°f for BrCl(g) is -1.0 kJ/mol and the standard molar entropy, S°, for BrCl(g) is 240.0 J/mol⋅K. Assume ΔH°f for N2O4(g) is -9.2 kJ/mol and ΔH°f for NO2(g) is 33.2 kJ/mol.

For the reaction A (g) ⇌ 2 B (g), K = 14.7 at 298 K, what is the value of the reaction quotient Q at 298 K when ΔG = 19.6 kJ/mol?

In the Haber process, ammonia is synthesized from N2 and H2. Given the reaction N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) and ΔG° at 298 K is –33.3 kJ/mol, what is the value of ΔG at 298 K for a reaction mixture with partial pressures of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3?