(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

Which state functions are required to understand the second law of thermodynamics?

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If the enthalpy change for the following reaction at $300 \ K$ is $+7 \ kJ \ mol^{-1}$,find the entropy change of the surrounding (in $J \ K^{-1}$)?
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$

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The unit of entropy is

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One mole of an ideal gas expands adiabatically and reversibly from its initial pressure to half of its initial pressure. What will be the value of $\Delta S$ in $J \ K^{-1} \ mol^{-1}$? $[\ln 2 = 0.693$ and $R = 8.314 \ J \ mol^{-1} \ K^{-1}]$

Medium

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Explain entropy and spontaneity.

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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

Which state functions are required to understand the second law of thermodynamics?

If the enthalpy change for the following reaction at $300 \ K$ is $+7 \ kJ \ mol^{-1}$,find the entropy change of the surrounding (in $J \ K^{-1}$)?$H_2O_{(s)} \longrightarrow H_2O_{(l)}$

The unit of entropy is

One mole of an ideal gas expands adiabatically and reversibly from its initial pressure to half of its initial pressure. What will be the value of $\Delta S$ in $J \ K^{-1} \ mol^{-1}$? $[\ln 2 = 0.693$ and $R = 8.314 \ J \ mol^{-1} \ K^{-1}]$

Explain entropy and spontaneity.

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If the enthalpy change for the following reaction at $300 \ K$ is $+7 \ kJ \ mol^{-1}$,find the entropy change of the surrounding (in $J \ K^{-1}$)?
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$