The standard enthalpies of formation of S(g), F(g), SF4(g), and

The standard enthalpies of formation of S(g), F(g), SF4(g), and SF6(g) are 1278.8 kJ/ mol, 179.0 kJ/ mol, –775 kJ/ mol, and –1209 kJ/ mol, respectively.
a. Use these data to estimate the energy of an SOF bond.
b. Compare the value that you calculated in part a with the value given in Table. What conclusions can you draw?
c. Why are the ΔHof values for S(g) and F(g) not equal to zero, even though sulfur and fluorine are elements?
Table
The standard enthalpies of formation of S(g), F(g), SF4(g), and

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