MCQ
Molar heat of vaporisation of a liquid is $6\,kJ\,mo{l^{ - 1}}$. If the entropy change is $16\,J\,mo{l^{ - 1}}\,{K^{ - 1}}$, the boiling point of the liquid is
- A${375\,^o}C$
- ✓$375\,K$
- C$273\,K$
- D${102\,^o}C$
✓
Answer
Correct option: B.
$375\,K$
(b)$\Delta S = 16\,J\,mol{e^{ - 1}}\,{K^{ - 1}}$
${T_{b.p.}} = \frac{{\Delta {H_{{\rm{vapour}}}}}}{{\Delta {S_{{\rm{vapour}}}}}} = \frac{{6 \times 1000}}{{16}} = 375\,K$
${T_{b.p.}} = \frac{{\Delta {H_{{\rm{vapour}}}}}}{{\Delta {S_{{\rm{vapour}}}}}} = \frac{{6 \times 1000}}{{16}} = 375\,K$
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