The standard enthalpies of formation of S(g), F(g), SF4(g), and SF6(g) are 1278.8 kJ/ mol, 179.0 kJ/
Question:
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
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a Using SF 4 data SF 4 g Sg 4 Fg H 4D SF 2788 kJ 4790 kJ 775 kJ 1370 Kj D SF 3425 kJmo...View the full answer
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