(A) The process is the fusion of ice: $H_2O_{(s)} \rightarrow H_2O_{(l)}$ at $T = 0 \ ^\circ C = 273 \ K$.The molar entropy change is $\Delta S_{fus}

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(A) The process is the fusion of ice: $H_2O_{(s)} \rightarrow H_2O_{(l)}$ at $T = 0 \ ^\circ C = 273 \ K$.The molar entropy change is $\Delta S_{fus} = S_{product} - S_{reactant} = 60 - 38.2 = 21.8 \ J/mol \ K$.For a reversible phase transition at equilibrium,$\Delta S = \frac{\Delta H}{T}$.Therefore,$\Delta H = \Delta S \times T = 21.8 \ J/mol \ K \times 273 \ K = 5951.4 \ J/mol$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

Medium

$18 \ g$ of ice is converted into water at $0 \ ^\circ C$ and $1 \ atm$. The entropies of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.2$ and $60 \ J/mol \ K$ respectively. The enthalpy change for this conversion is ..... $J/mol$.

A
$5951.4$
B
$595.14$
C
$-5951.4$
D
$2975.7$

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2 nd Law of thermodynamics and Entropy

The standard entropies of $CO_{2(g)}$,$C_{(s)}$ and $O_{2(g)}$ are $213.5$,$5.690$ and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is ...... $J \ K^{-1} \ mol^{-1}$.

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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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For which one of the following reactions is the entropy change positive?

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Standard entropy of $X_2, Y_2$ and $XY_3$ are $60, 40$ and $50 \ J \ K^{-1} \ mol^{-1},$ respectively. For the reaction,$\frac{1}{2}X_2 + \frac{3}{2}Y_2 \to XY_3, \ \Delta H = -30 \ kJ,$ to be at equilibrium,the temperature will be ............... $K$.

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$18 \ g$ of ice is converted into water at $0 \ ^\circ C$ and $1 \ atm$. The entropies of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.2$ and $60 \ J/mol \ K$ respectively. The enthalpy change for this conversion is ..... $J/mol$.

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The standard entropies of $CO_{2(g)}$,$C_{(s)}$ and $O_{2(g)}$ are $213.5$,$5.690$ and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is ...... $J \ K^{-1} \ mol^{-1}$.

State the limitation of the $2^{nd}$ law of thermodynamics.

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

For which one of the following reactions is the entropy change positive?

Standard entropy of $X_2, Y_2$ and $XY_3$ are $60, 40$ and $50 \ J \ K^{-1} \ mol^{-1},$ respectively. For the reaction,$\frac{1}{2}X_2 + \frac{3}{2}Y_2 \to XY_3, \ \Delta H = -30 \ kJ,$ to be at equilibrium,the temperature will be ............... $K$.

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