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Question

The heat of combustion of acetylene is 312 kcal. If heat of formation of CO2 and H2O are 94.38 and 68.38 kcal respectively, CC bond energy is xkcal. Given that heat of atomisation of C and H are 150.0 and 51.5 kcal respectively and CH bond energy is 93.64 kcal. Value of x

A
161
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B
150
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C
170
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D
None of these
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Solution

The correct option is A 161
Given,
C2H2+(5/2)O22CO2+H2O;ΔH=312kcal ... (i)
( Heat of combustion are exothermic)
C+O2CO2;ΔH=94.38kcal ... (ii)
H2+12O2H2O;ΔH=68.38kcal ... (iii)

Multiply eq. (ii) by 2 and add in eq. (iii)


2C+H2+(5/2)O22CO2+H2O;ΔH=257.14kcal ...( iv)

Subtracting eq. (i) from eq. (iv)

C2H2+(5/2)O22CO2+H2O;ΔH=312kcal ...( i)
- - - - +
........................................................................................................................
2C+H2C2H2;ΔH=+54.86kcal ... (v)

Also ΔH for C+H2C2H2

ΔH=Bondenergydataofformationofbond+Bondenergydataofdissociationofbond
ΔH=[e(CC)+2×e(CH)]+[2Csg+e(HH)]

Also given, Csg=150kcal
12H2(g)H(g)51.5kcal

eHH=51.5×2kcal=103.0kcal
eCH=93.64kcal

54.86=[e(CC)+2×93.64]+[2×150+1×103.0]

eCC=160.86kcal

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