O₂ at 293 K, partial pressure = 0.98 bar, KH = 34 kbar. Find solubility in g/L.

Step-1: Mole fraction:

x(O₂) = 0.98 / 34000 = 2.882×10⁻⁵

Step-2: Moles of O₂ in 1 L:

n(O₂) ≈ 2.882×10⁻⁵ × 55.5 = 1.60×10⁻³ mol

Step-3: Mass (Mᵣ of O₂ = 32 g/mol):

mass = 1.60×10⁻³ × 32 = 0.0512 g

Answer: Solubility of O₂ ≈ 0.0512 g/L

O₂ has a smaller KH than N₂ (34 vs 76.48 kbar) meaning O₂ is more soluble, which is why aquatic life can survive using dissolved O₂.