The enthalpy of fusion of water is 1.435 kca | vedclass

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

Question

(C) The process of melting ice at $0 \ ^\circ C$ $(273 \ K)$ is a reversible phase transition.For a reversible process,the entropy change is given by

Vedclass · Accepted Answer

$5.260 \ cal/(mol \ K)$

Vedclass · Answer

(C) The process of melting ice at $0 \ ^\circ C$ $(273 \ K)$ is a reversible phase transition.For a reversible process,the entropy change is given by $\Delta S = \frac{\Delta H_{fus}}{T}$.Given $\Delta H_{fus} = 1.435 \ kcal/mol = 1435 \ cal/mol$.Temperature $T = 0 \ ^\circ C = 273 \ K$.Therefore,$\Delta S = \frac{1435 \ cal/mol}{273 \ K} = 5.256 \ cal/(mol \ K) \approx 5.26 \ cal/(mol \ K)$.

The enthalpy of fusion of water is $1.435 \ kcal/mol$. The molar entropy change for the melting of ice at $0 \ ^\circ C$ is

Similar Questions

$A$ boiled egg shows entropy:

What is the change in entropy when an ideal gas expands into a vacuum?

Identify the correct statement regarding a spontaneous process:

The entropy change when $2 \, \text{moles}$ of an ideal monoatomic gas is heated from $200 \, ^\circ \text{C}$ to $300 \, ^\circ \text{C}$ isochorically is:

For a spontaneous process,the correct statement is

Vedclass Test Series

Exam Paper Generator

Online Exam Module