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Answer :
The enthalpy of the sublimation of sodium can be calculated by adding the enthalpy of fusion and the enthalpy of vaporization. Using the given information for sodium, with an enthalpy of fusion of 2.6 kJ/mol and an enthalpy of vaporization of 98.2 kJ/mol, the enthalpy of sublimation can be estimated as the sum of these two values. Therefore, the calculated enthalpy of sublimation for sodium would be 100.8 kJ/mol (2.6 kJ/mol + 98.2 kJ/mol).
Similarly, for the unknown organic substance with a provided molar enthalpy of sublimation of 58.05 kJ/mol and a molar enthalpy of vaporization of 37.12 kJ/mol, the molar enthalpy of fusion can be estimated by subtracting the enthalpy of vaporization from the enthalpy of sublimation. Thus, the enthalpy of fusion for the unknown substance is approximately 20.93 kJ/mol (58.05 kJ/mol - 37.12 kJ/mol).
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