The molar enthalpy of solidification of pure sulfur is -4.123 kJ/mol.
If you want to get the correct sign for the molar entropy of solidification, you must use the formulas
heat lost by sulfur = -heat gained by the calorimeter
moles × molar heat = -mass × specific heat capacity × change in temperature
In symbols, these become
Here are the numbers we have to insert into the formulas.
Since your numbers are all given to 4 significant figures, we must use the mass of water to 4 significant figures.
The density of water at 32.40 °C is 0.9943 g/mL.
The specific heat capacity of water is
This gives us
∴ The molar enthalpy of solidification of sulfur is -4.123 kJ/mol.
The negative sign tells us that the sulfur loses heat energy when it solidifies.
NOTE: There is either an error in your data or in my calculations, because the molar entropy of solidification of sulfur is -1.727 kJ/mol.