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Question

Using the following thermochemical data,
C(s)+O2(g)CO2(g) ΔH=94.0 kcal
H2(g)+12O2(g)H2O(l) ΔH=68.0 kcal
CH3COOH(l)+2O2(g)2CO2(g)+2H2O(l) ΔH=210.0 kcal
the heat of formation of acetic acid is :

A
116 kcal
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B
-116 kcal
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C
-114 kcal
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D
114 kcal
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Solution

The correct option is C -114 kcal
Given reactions are C(s)+O2(g)CO2(g) ΔH=94.0 kcal....(1)

H2(g)+12O2(g)H2O(l) ΔH=68.0 kcal...(2)

CH3COOH(l)+2O2(g)2CO2(g)+2H2O(l) ΔH=210.0 kcal....(3)

reversing the reaction 3, we get
2CO2(g)+2H2O(l)CH3COOH(l)+2O2(g) ΔH=+210.0 kcal....(4)

multiplying equation (1) and (2) by 2 we get,
2C(s)+2O2(g)2CO2(g) ΔH=2×94.0 kcal........5
2H2(g)+O2(g)2H2O(l) ΔH=2×68.0 kcal.......6

Add eqn. 4, 5 and 6 to obtain
2C(s)+2H2(g)+O2(g)CH3COOH(l)

so the heat of formation of acetic acid =210.0+2(94.0)+2(68.0)
=114 kcal

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