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Answer :
Final answer:
The enthalpy calculations for sodium involve fusion and vaporization processes, resulting in specific enthalpy values for each transformation.
Explanation:
The total enthalpy change when 1 mol of sodium is converted from solid to vapor: To calculate this, you need to add the enthalpy of fusion and enthalpy of vaporization. For sodium, it would be 2.6 kJ/mol (fusion) + 98.2 kJ/mol (vaporization) = 100.8 kJ/mol.
The enthalpy change when 1 mol of sodium is melted and then vaporized: This would be the sum of the enthalpies of fusion and vaporization, which is 100.8 kJ/mol.
The enthalpy change when 1 mol of sodium is vaporized: In this case, it would be the enthalpy of vaporization only, which is 98.2 kJ/mol for sodium.
The enthalpy change when 1 mol of sodium is melted: This would be the enthalpy of fusion, which is 2.6 kJ/mol for sodium.
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