Calculate the entropy change in melting 1 mole of ice at 273 ~K, Δ H_f^o=6.025 ~kJ / mole-

Correct answer: (B) 22.1 ~J ~K^-1 ~mol^-1. Δ S_f=fracΔ H_fT=frac6025 ~J ~mol^-1273 ~K=22.1 JK^-1 mol^-1

Q24 / 120 · VITEEE 2019 · Chemistry

Calculate the entropy change in melting 1 mole of ice at $273 \mathrm{~K}, \Delta \mathrm{H}_{\mathrm{f}}^{\mathrm{o}}=6.025 \mathrm{~kJ} /$ mole-

A
$11.2 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$
Correct answer
B
$22.1 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$
C
$15.1 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$
D
$5.1 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$

Solution

$\Delta \mathrm{S}_{\mathrm{f}}=\frac{\Delta \mathrm{H}_{\mathrm{f}}}{\mathrm{T}}=\frac{6025 \mathrm{~J} \mathrm{~mol}^{-1}}{273 \mathrm{~K}}=22.1 \mathrm{JK}^{-1}$ $\mathrm{mol}^{-1}$

Hence, the correct answer is option: 'B'.

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