Calculate the total energy required to convert a 11.5 g solid piece of sodium metal completely into gaseous Na ⁺ ions. The total energy absorbed is _______ kJ . [Given: Enthalpy of sublimation of Na = 108 kJ mol ⁻¹ , First ionization enthalpy of Na = 496 kJ mol ⁻¹ , Molar mass of Na = 23 g mol ⁻¹ ]

Step-by-step solution

The conversion of solid sodium to gaseous sodium ions involves two steps: sublimation of solid sodium to gaseous sodium atoms, followed by the ionization of gaseous sodium atoms. Total energy required per mole = _ sub H + IE₁ = 108 + 496 = 604 kJ mol ⁻¹ Number of moles of sodium = 11.5 g 23 g mol ⁻¹ = 0.5 mol Total energy required for 0.5 mol of Na = 0.5 mol 604 kJ mol ⁻¹ = 302 kJ Answer: 302