Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IICalculation of DSMedium2 minPYQ_2023

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$30.4 kJ$ of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is $28.4 J K^{- 1} {mol}^{- 1}$ at $1 atm$ . The melting point of sodium chloride is _______ $K$ (Nearest Integer)

Answer:

1070

Solution:

The equilibrium process can be written as follows,

$\begin{array}{l} NaCl (s) \overset{}{⇌} NaCl (l) \\ ΔS = \frac{ΔH}{Temp} \\ T = \frac{ΔH}{ΔS} \\ = \frac{30 .4 \times 10^{3}}{28 .4} \\ = 1070 .4 K \end{array}$

Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:Calculation of DS

⏱ 2mℹ️ Source: PYQ_2023

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