(B) At equilibrium,the process of melting ice to water occurs at $273 \, K$ where $\Delta G = 0$. Using the Gibbs-Helmholtz equation: $\Delta G = \Del

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(B) At equilibrium,the process of melting ice to water occurs at $273 \, K$ where $\Delta G = 0$. Using the Gibbs-Helmholtz equation: $\Delta G = \Delta H - T \Delta S$. Since $\Delta G = 0$,we have $\Delta H = T \Delta S$. Here,$\Delta S = S_{(l)} - S_{(s)} = 60.01 - 38.20 = 21.81 \, J \, mol^{-1} \, K^{-1}$. Therefore,$\Delta H = 273 \, K \times 21.81 \, J \, mol^{-1} \, K^{-1} = 5954.13 \, J \, mol^{-1}$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

Medium

One mole of ice is converted into water at $273 \, K$. The entropy of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.20 \, J \, mol^{-1} \, K^{-1}$ and $60.01 \, J \, mol^{-1} \, K^{-1}$ respectively. The enthalpy change for the conversion is $....... \, J \, mol^{-1}$.

A
$4690.81$
B
$5954.13$
C
$3945.23$
D
$4125.90$

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Class 11

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Thermodynamics

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2 nd Law of thermodynamics and 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?
$H_2O_{(l)} \to H_2O_{(g)}$ ... $J \, K^{-1} \, mol^{-1}$

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The entropy change involved in the isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

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The $\Delta S$ for the vaporisation of $1 \ mol$ of water is $88.3 \ J/mol \ K$. The value of $\Delta S$ for the condensation of $1 \ mol$ of vapour will be.......$ J/mol \ K$

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According to the second law of thermodynamics,which of the following is true for a spontaneous process?

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Which of the following statements is correct?

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One mole of ice is converted into water at $273 \, K$. The entropy of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.20 \, J \, mol^{-1} \, K^{-1}$ and $60.01 \, J \, mol^{-1} \, K^{-1}$ respectively. The enthalpy change for the conversion is $....... \, J \, mol^{-1}$.

Similar Questions

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 isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

The $\Delta S$ for the vaporisation of $1 \ mol$ of water is $88.3 \ J/mol \ K$. The value of $\Delta S$ for the condensation of $1 \ mol$ of vapour will be.......$ J/mol \ K$

According to the second law of thermodynamics,which of the following is true for a spontaneous process?

Which of the following statements is correct?

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