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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 kJWE know, △Go=−2.303 RT log K putting the values =−2.303×8.314×298 log (1.3×103) =−17767.688 J mol−1=−17.767 kJ mol−1 We also know that, △Go=△Ho−T△So putting the values −17.767=−66.5−298×△So △So=−66.5+17.767298=−0.163 kJ mol−1 K−1

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