Question

The most common form of elemental sulfur is S8, in which eight sulfur atoms linked in a ring of single bonds. At high temperature, 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).

Answer 1

Step-by-step explanation:

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

Given

1920 + 4x = 239

4x = 239 - 1920

x = - 420.25 kJ .

So bond energy of S₂ = 420.25 kJ .