(A) For a phase transition at equilibrium,the entropy change is given by the formula:$\Delta S = \frac{\Delta_{vap} H}{T_{BP}}$Given $\Delta_{vap} H =

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(A) For a phase transition at equilibrium,the entropy change is given by the formula:$\Delta S = \frac{\Delta_{vap} H}{T_{BP}}$Given $\Delta_{vap} H = 39.2 \, kJ \, mol^{-1} = 39.2 \times 10^3 \, J \, mol^{-1}$ and $T = 373 \, K$.Substituting the values:$\Delta S = \frac{39.2 \times 10^3}{373} \approx 105.09 \, J \, K^{-1} \, mol^{-1}$.Rounding to the nearest integer,we get $105 \, J \, K^{-1} \, mol^{-1}$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

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

A
$105$
B
$31$
C
$21.98$
D
$326$

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Thermodynamics

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2 nd Law of thermodynamics and Entropy

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:

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In which of the following processes is $\Delta S$ positive?

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For the following process $H_2O_{(l)} (1 \ bar, 373.15 \ K) \rightleftharpoons H_2O_{(g)} (1 \ bar, 373.15 \ K)$, identify the correct set of thermodynamic parameters.

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The enthalpy of vaporization of water at $298 \ K$ is $386 \ kJ \ mol^{-1}$. What is the entropy of vaporization of water in $kJ \ K^{-1} \ mol^{-1}$?

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In a reversible expansion,one mole of gas is expanded isothermally at $200 \ K$ till its volume increases $10$ times. Calculate $\Delta S_{total}$ at equilibrium (in $J \ K^{-1}$)?

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

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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:

In which of the following processes is $\Delta S$ positive?

For the following process $H_2O_{(l)} (1 \ bar, 373.15 \ K) \rightleftharpoons H_2O_{(g)} (1 \ bar, 373.15 \ K)$, identify the correct set of thermodynamic parameters.

The enthalpy of vaporization of water at $298 \ K$ is $386 \ kJ \ mol^{-1}$. What is the entropy of vaporization of water in $kJ \ K^{-1} \ mol^{-1}$?

In a reversible expansion,one mole of gas is expanded isothermally at $200 \ K$ till its volume increases $10$ times. Calculate $\Delta S_{total}$ at equilibrium (in $J \ K^{-1}$)?

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