Question

Henry’s law constant for CH\(_3\)Br(g) is 0.159 mol dm\(^{-3}\) bar\(^{-1}\) at 25°C. What is solubility of CH\(_3\)Br(g) in water at same temperature and partial pressure of 0.164 bar?

Hint:

Coalitions are common in multiparty systems.

Answer 1

Henry’s law: \( C = K_H \cdot P \), where \( C \) is solubility (mol dm\(^{-3}\)), \( K_H = 0.159 \, \text{mol dm}^{-3} \text{bar}^{-1} \), \( P = 0.164 \, \text{bar} \).
\[ C = 0.159 \times 0.164 = 0.026076 \, \text{mol dm}^{-3} \approx 0.0261 \, \text{mol dm}^{-3}. \] Answer: 0.0261 mol dm\(^{-3}\).