Enthalpy of sublimation of iodine is $24\,{\rm{cal}}\,{g^{ - 1}}$ at ${200^{\rm{o}}}C$. If specific heat of ${I_2}\left( s \right)$ and ${I_2}\left( {{\rm{vap}}{\rm{.}}} \right)$ are 0.055 and 0.031 ${\rm{cal }}{g^{ - 1}}{K^{ - 1}}$ respectively, then enthalpy of sublimation of iodine at ${250^{\rm{o}}}C$ in ${\rm{cal}}\,{g^{ - 1}}$ is

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

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Application +4 | -1

Enthalpy of sublimation of iodine is

24\,\mathrm{cal}\,{g^{ - 1}}

{200^\mathrm{o}}C

. If specific heat of

{I_2}\left( s \right)

and

{I_2}\left( {\mathrm{vap}\mathrm{.}} \right)

are 0.055 and 0.031

\mathrm{cal }{g^{ - 1}}{K^{ - 1}}

respectively, then enthalpy of sublimation of iodine at

{250^\mathrm{o}}C

\mathrm{cal}\,{g^{ - 1}}

View answer and explanation

Correct option: C

22.8

Option C (22.8) is correct because it is calculated using Kirchhoff's equation to account for the temperature change.

Practice All Chapter MCQs →

{T_i}

{T_f}

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

\Delta G