The most common form of elemental sulfur is S8, in which eight sulfur atoms linked in a ring of single bonds. At high temperatur
e, in the gas phase, S8 can break apart to give S2, the sulfur analog of molecular oxygen: S8(g) 4S2(g) ΔH = +239 kJ at T = 800 K
Using the appropriate data in Table 3-2 S-S 240 calculate the S=S double-bond energy (in kJ/mol) in S2(g).
In S₈ , there are 8 single bonds which breaks up first . Energy absorbed
= 8 x 240 = 1920 kJ
In S₈ four double bonds of S₂ are formed . Let bond energy be x . In this process energy will be released . energy released in four S₂ molecules formed = 4 x
They discovered this since S waves don’t travel through the earth but P waves do. P waves tend to travel faster than S waves in speed, 1&14km/s vs 1&8km/s
