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Q.

The heat of combustion of ethene gas is ΔHc=-330   Kcal/mol calculate >C=C< Bond energy (in kcal/mol) assuming that the bond energy of the C-H bond is 93.6 Kcal/mol
Given: ΔHf0for  CO2(g)  and  H2O(l)are  94.2  and  61Kcalmol1 Respectively.  ΔHa(C(s))=150k.cal.mol1,  ΔHf(H(g))=51.5k.cal.mol1

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answer is 112.

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Detailed Solution

 B.E(C=C)=112  Kcal/mol CH2=CH2(g)+3O2(g)2CO2(g)+2H2O(f) 330=[2×(94.2)+2(61)][ΔHf+C2H4]        ΔHf+(C2H4)=19.6  Kcal  mol1 2C(s)+2H2(g)CH2=CH2(g);ΔHf=19.6 ΔHReaction=2ΔHatm(C)+4ΔHatm(H)4B.E.(CH)B.E.(CC) 19.6=2×150+4×51.54×93.6B.E.(CC) B.E.(CC)=112  Kcal/mol

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