1. Write the Balanced Chemical Equation:

The reaction of sulfur with oxygen produces sulfur dioxide:

S(s) + O₂(g) → SO₂(g)

2. Determine the Molar Mass of Sulfur:

The molar mass of sulfur (S) is 32.06 g/mol.

3. Calculate the Moles of Sulfur:

Moles of sulfur = (mass of sulfur) / (molar mass of sulfur)

Moles of sulfur = 6.44 g / 32.06 g/mol

Moles of sulfur ≈ 0.201 mol

4. Determine the Enthalpy Change of the Reaction (ΔH):

The standard enthalpy change of formation (ΔHf°) for sulfur dioxide (SO₂) is -296.8 kJ/mol. This means that 296.8 kJ of heat is released when one mole of SO₂ is formed.

5. Calculate the Heat Released:

Since the reaction releases heat, the enthalpy change is negative. The heat released is directly proportional to the moles of sulfur reacting.

Heat released = (moles of sulfur) × (ΔH)

Heat released = (0.201 mol) × (-296.8 kJ/mol)

Heat released ≈ -59.7 kJ

Therefore, approximately 59.7 kJ of heat will be released when 6.44 grams of sulfur reacts with excess oxygen.