At -10°C, the solid compound Cl₂(H₂O)₈ is in equilibrium with gaseous chlorine, water vapour and ice — Chemical Equilibrium Chemistry Question
Question
At -10°C, the solid compound Cl₂(H₂O)₈ is in equilibrium with gaseous chlorine, water vapour and ice. The partial pressure of the two gases in equilibrium with a mixture of Cl₂(H₂O)₈ and ice are 0.20 atm for Cl₂ and 0.001 atm for water vapour. The processes may be represented as:<br>(i) Cl₂(H₂O)₈(s) ⇌ Cl₂(g) + 8H₂O(g); K_{p_1}<br>(ii) Cl₂(H₂O)₈(s) ⇌ Cl₂(g) + 8H₂O(s); K_{p_2}<br>Identify the correct statement among the following regarding the processes.
💡 Solution & Explanation
For process (i), K_{p_1} = P_Cl₂ × (P_H₂O)⁸ = 0.20 × (0.001)⁸ = 2.0 × 10⁻²⁵ atm⁹. For process (ii), since water is solid ice, K_{p_2} = P_Cl₂ = 0.20 atm. The equilibrium vapour pressure of ice is given directly by the partial pressure of water vapour, which is 0.001 atm at -10°C (263 K). Dissociation processes like (i) are generally endothermic, not exothermic. Therefore, correct answer is A,B,C.