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Question

The enthalpy of SS bond from the following data is:


( i ) C2H5SC2H5(g);ΔfHo=147.2 kJ / mol

( ii ) C2H5SSC2H5(g);ΔfHo=201.9 kJ / mol

( iii ) S(g);ΔfHo=222.8 kJ / mol

A
124.5 kJ / mol
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B
887.5 kJ / mol
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C
967.5 kJ / mol
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D
277.5 kJ / mol
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Solution

The correct option is D 277.5 kJ / mol
Given;
(i) 4C(s)+5H2(g)+S(s)C2H5SC2H5(g) ΔfH=147.23kJ/mol
(ii) 4C(s)+5H2(g)+2S(s)C2H5SSC2H5(g) ΔfH=201.92kJ/mol
(ii)(i) gives
C2H5SC2H5(g)+S(s)C2H5SSC2H5(g)
ΔfH=201.92+147.23=54.69kJ/mol
Add the above equation to the following equation
S(g)S(s) ΔfH=222.80kJ/mol to get,
C2H5SC2H5(g)+S(g)C2H5SSC2H5(g)
ΔfH=222.80+(54.69)=277.49kJ/mol
This heat is evolved because of formation of SS bond.
So, bond enthapy of SS is 277.49kJ/mol

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