BaCl2 ∙ H2O(s) loses water when it is heated in an oven:
BaCI2 ∙ H2O (s) ⇌ BaCl2(s) + H2O(g)
∆H° = 63.11 kJ/mol at 25°C
∆S° = + 148J(K ∙ mol) at 25°C
(a) Write the equilibrium constant for this reaction. Calculate the vapor pressure of gaseous H2O (PH2O)above BaCl2 ∙ H2O at 298 K.
(b) If ∆H° and ∆S° are not temperature dependent (a poor assumption), estimate the temperature at which PH2O above BaCl2 ∙ H2O(s) will be 1 bar. H2O(s) will be 1 bar.