Assertion : Entropy of ice is less than water | vedclass

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

Question

(A) Entropy is a measure of the degree of randomness or disorder in a system.In the solid state (ice),molecules are held in a fixed,ordered lattice,wh

Vedclass · Accepted Answer

If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

Vedclass · Answer

(A) Entropy is a measure of the degree of randomness or disorder in a system.In the solid state (ice),molecules are held in a fixed,ordered lattice,whereas in the liquid state (water),molecules have more freedom of movement.Therefore,the entropy of ice is less than that of water.The reason provided,that ice has an open cage-like structure due to hydrogen bonding,is also a correct statement.This cage-like structure restricts the movement of water molecules,which is the underlying cause for the lower entropy of ice compared to water.Thus,the Reason correctly explains the Assertion.

Assertion : Entropy of ice is less than water.
Reason : Ice has a cage-like structure.

Similar Questions

Entropy is maximum in case of

$18 \ g$ of ice is converted into water at $0 \ ^\circ C$ and $1 \ atm$. The entropies of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.2$ and $60 \ J/mol \ K$ respectively. The enthalpy change for this conversion is ..... $J/mol$.

State the characteristics of 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?
$H_2O_{(l)} \to H_2O_{(g)}$ ... $J \, K^{-1} \, mol^{-1}$

The entropy change involved in the conversion of $1 \, \text{mole}$ of liquid water at $373 \, K$ to vapour at the same temperature will be $[\Delta H_{vap} = 2.257 \, kJ/g]$. (in $, kJ/K$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Assertion : Entropy of ice is less than water.Reason : Ice has a cage-like structure.