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Question

Acetic acid CH3COOH can form a dimer (CH3COOH)2 in the gas phase. The dimer is held together by two H-bonds with a total strenght of 66.5 kJ per mol of dimer
If at 25oC, the equilibrium constant for the dimerization is 1.3×103. Calculate So for the reaction:
2CH3COOH(g)(CH3COOH)2(g)

A
0.263 kJ
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B
0.463 kJ
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C
0.163 kJ
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D
0613 kJ
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Solution

The correct option is C 0.163 kJ
WE know,
Go=2.303 RT log K
putting the values
=2.303×8.314×298 log (1.3×103)
=17767.688 J mol1=17.767 kJ mol1

We also know that,
Go=HoTSo
putting the values
17.767=66.5298×So
So=66.5+17.767298=0.163 kJ mol1 K1

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