Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + 1/2 O₂(g) ⇌ NO₂(g) (2) 2 NO₂(g) ⇌ 2 NO(g) + O₂(g) Which one of the following is the correct relationship between the equilibrium constants K₁ and K₂? A) K₂ = –K₁/2 B) K₂ = 1/(2K₁) C) K₂ = 1/(2K₁)² D) K₂ = 2/K₁ E) K₂ = (1/K₁)² Solution: What do we need to do to equation 1 to turn it into equation 2. Let's look at NO. To go to the second equation, we need to multiply NO by 2 and revers

Predict the sign of ∆Ssys for the following processes. a) N₂(g) → 2 N(g) b) K(l) → K(s) c) 3 O₂(g) → 2 O₃(g) d) CaCO₃(s) → CaO(s) + CO₂(g) e) Compressing 5.0 L of Cl₂(g) to 1.0 L (constant temperature) f) Heating steam from 100 °C to 200 °C Solution: The change in entropy, ΔS, represents the degree of disorder in a system. When looking at an equation there are two things you have to look for to predict the sign of ∆S. Phases (gas,liquid, solid) going from reactants to product