The enthalpy values for the following reactions are:

4C(s) + 4H₂(g) → C₄H₈(g) ΔH = – 7.1 kJ/mol
½4C(s) + 5H₂(g) + ½O₂(g) → C₄H₁₀O(g) ΔH = – 292.8 kJ/mol
2H₂(g) + O₂(g) → 2H₂O(g) ΔH = – 483.6 kJ/mol

Using the data above, calculate the enthalpy change, in kJ mol–1, for the production of butan-2-ol by hydration of but-2-ene:

C₄H₈(g) + H₂O(g) → C₄H₁₀O(g)