19. Chemical Thermodynamics

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.

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.

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?

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?

A redox reaction has an equilibrium constant of K = 1.2 x 10^3. Which statement is true regarding ΔG°_rxn and E°_cell for this reaction?