Chemistry · 2017
JEE Main · 8 April 2017, Shift 1 · Q40
The enthalpy change on freezing of 1 mol of water at 5°C to ice at -5°C is: (Given Δ_fus H =6 kJ mol^-1 at 0°C, C_p ( H_2 O, l)=75.3 J mol^-1 K^-1,.…
The enthalpy change on freezing of $\displaystyle 1$ mol of water at $\displaystyle 5$°C to ice at -$\displaystyle 5$°C is :
(Given $\displaystyle \Delta_{\text {fus }} \mathrm{H}=6 \mathrm{~kJ} \mathrm{~mol}^{-1}$ at $\displaystyle 0$°C, $\displaystyle \mathrm{C}_{\mathrm{p}}\left(\mathrm{H}_2 \mathrm{O}, l\right)=75.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$, $\displaystyle \left.\mathrm{C}_{\mathrm{p}}\left(\mathrm{H}_2 \mathrm{O}, \mathrm{s}\right)=36.8 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$
Official answer
(3)
$\displaystyle 6.56 \mathrm{~kJ} \mathrm{~mol}^{-1}$
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JEE Main 2017 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.