One mole of ice is converted into water at 1 | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The process is the phase transition of ice to water at its melting point: $H_2O_{(s)} \longrightarrow H_2O_{(\ell)}$.At equilibrium,the change in

Vedclass · Accepted Answer

$5954$

Vedclass · Answer

(B) The process is the phase transition of ice to water at its melting point: $H_2O_{(s)} \longrightarrow H_2O_{(\ell)}$.At equilibrium,the change in entropy is given by $\Delta S = \frac{\Delta H}{T}$.Given $\Delta S = S_{H_2O(\ell)} - S_{H_2O(s)} = 60.01 - 38.2 = 21.81 \ J \ mol^{-1} \ K^{-1}$.Given temperature $T = 273 \ K$.Therefore,$\Delta H = \Delta S 	imes T = 21.81 	imes 273 = 5954.13 \ J \ mol^{-1}$.

One mole of ice is converted into water at $1 \ atm$ and $273 \ K$. The entropies of $H_2O_{(s)}$ and $H_2O_{(\ell)}$ are $38.2$ and $60.01 \ J \ mol^{-1} \ K^{-1}$ respectively. The enthalpy change for the conversion is ...... $J \ mol^{-1}$.

Similar Questions

Which of the following is the least $random$ state of water?

For which of the following reactions will $\Delta S$ be maximum?

What is entropy?

At $373 \, K$,steam and water are in equilibrium and $\Delta H = 39.2 \, kJ \, mol^{-1}$. What will be $\Delta S$ for the conversion of $1 \, mole$ of water into steam?
$H_2O_{(l)} \to H_2O_{(g)}$ ... $J \, K^{-1} \, mol^{-1}$

In which of the following reactions is $\Delta S$ maximum?

Vedclass Test Series

Exam Paper Generator

Online Exam Module