The standard enthalpy of solution of AgCl (s) is +65 ~kJ/mol . If the standard enthalpies of formation of Ag ^+(aq) and Cl ^-(aq) are +105 ~kJ/mol and -167 ~kJ/mol respectively, the standard enthalpy of formation of AgCl (s) in kJ/mol is :

Step-by-step solution

The dissolution of silver chloride in water is represented by the equation: AgCl (s) Ag ^+(aq) + Cl ^-(aq) According to Hess's Law, the standard enthalpy of solution is given by the difference between the sum of the standard enthalpies of formation of the products and the reactant: H_ sol ^ = [ H_f^ ( Ag ^+) + H_f^ ( Cl ^-)] - H_f^ ( AgCl ) Substituting the given values: +65 = [+105 + (-167)] - H_f^ ( AgCl ) 65 = -62 - H_f^ ( AgCl ) Rearranging to solve for the standard enthalpy of formation of AgCl (s) : H_f^ ( Ag