One mole of ice is converted into water at 273 K. The entropies of $\;{{\rm{H}}_2}{\rm{O}}$ (S) and $\;{{\rm{H}}_2}{\rm{O}}$ (l)are 38.20 and 60.01 J ${\rm{mo}}{{\rm{l}}^{ - 1}}{{\rm{K}}^{ - 1}}$ respectively. The enthalpy change for the conversion is:

$5954{\rm{Jmo}}{{\rm{l}}^{ - 1}}$

$59.54{\rm{Jmo}}{{\rm{l}}^{ - 1}}$

$595.4{\rm{Jmo}}{{\rm{l}}^{ - 1}}$

$320.6{\rm{Jmo}}{{\rm{l}}^{ - 1}}$

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NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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One mole of ice is converted into water at 273 K. The entropies of

\;{\mathrm{H}_2}\mathrm{O}

(S) and

\;{\mathrm{H}_2}\mathrm{O}

(l)are 38.20 and 60.01 J

\mathrm{mo}{\mathrm{l}^{ - 1}}{\mathrm{K}^{ - 1}}

respectively. The enthalpy change for the conversion is:

View answer and explanation

Correct option: B

5954\mathrm{Jmo}{\mathrm{l}^{ - 1}}

Option B (5954 Jmol⁻¹) is correct because the enthalpy change is calculated by multiplying the temperature by the change in entropy during the phase transition.

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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