For the reaction A(g) ⇌ B(g) with ΔG° = 31.5 kJ at 298K, if the initial concentration of A is 0.100 M, what is the equilibrium concentration of B?

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?

Using standard free energy of formation values, calculate the equilibrium constant Kp for the reaction Cl2(g) + 2NO(g) ↔ 2NOCl(g) at 298 K. Given that the standard free energy change (ΔG°) for the reaction is -33.0 kJ/mol, what is the value of Kp?

What is the relationship between the equilibrium constant (Kₚ), the reaction quotient (Qₚ), and the standard equilibrium constant (K₀) for a reaction involving gases?

When adjusted for any changes in ΔH and ΔS with temperature, the standard free energy change ΔG°T at 2400 K is equal to 1.22×10^5 J/mol. Calculate the equilibrium constant (K) at 2400 K.