Consider the reaction: N₂(g)+ 3 X₂(g)→ 2 NX₃(g) △_fH° (kJ/mol)0.0 0.0 43 S° (J/(mol K))192 210 172 What is K_eq for this reaction at 591 K? A)2.3 × 10¹⁷ B)4.3 × 10^-18 C)1.04 D)0.96 E)132

Question

Quizplus · Accepted Answer

The equilibrium constant K_eq can be calculated using the Gibbs free energy change (ΔG°) and the relation ΔG° = -RT ln(K_eq). First, calculate ΔG° using ΔG° = ΔH° - TΔS°, where ΔH° and ΔS° are derived from the given formation enthalpies and entropies. The calculated ΔG° is positive, indicating a non-spontaneous reaction, leading to a very small K_eq value.

Consider the Reaction: N2(g)+ 3 X2(g)→ 2 NX3(g)

Consider the Reaction: N₂(g)+ 3 X₂(g)→ 2 NX₃(g)