The formation of sulfur trioxide from sulfur dioxide and oxygen proceeds according to
2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) ΔG° = –141 kJ mol⁻¹ (per overall reaction as written) at 298 K.
A mixture at 298 K in a 10.0 L rigid container contains the following partial pressures:
SO₂ = 0.200 atm, O₂ = 0.100 atm, SO₃ = 2.00 atm.
(The gas constant R = 8.314 J mol⁻¹ K⁻¹.)
(1) Calculate the reaction quotient, Q, for the forward reaction using the partial pressures given.
(2) Determine the Gibbs free energy change, ΔG, for the reaction under the specified conditions. Report your answer in kJ to three significant figures.
(3) State whether the forward reaction is thermodynamically favored, unfavored, or at equilibrium under these conditions, and justify your choice based on the value of ΔG.