(C) For a reaction to be spontaneous according to the $2^{nd}$ law of thermodynamics: $\Delta G < 0$. Since $\Delta G = \Delta H - T \Delta S$,we have

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(C) For a reaction to be spontaneous according to the $2^{nd}$ law of thermodynamics: $\Delta G Since $\Delta G = \Delta H - T \Delta S$,we have $\Delta H - T \Delta S At equilibrium,$\Delta G = 0$,so $\Delta H = T_e \Delta S$,which implies $T_e = \frac{\Delta H}{\Delta S}$. For the reaction to be spontaneous,$\Delta H - T \Delta S \Delta H$. Since $\Delta S$ is positive,$T > \frac{\Delta H}{\Delta S}$. Therefore,$T > T_e$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

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Let us consider a reversible reaction at temperature,$T$. In this reaction,both $\Delta H$ and $\Delta S$ were observed to have positive values. If the equilibrium temperature is $T_e$,then the reaction becomes spontaneous at:

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A
$T = T_e$
B
$T_e > T$
C
$T > T_e$
D
$T_e = 5 \ T$

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2 nd Law of thermodynamics and Entropy

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Considering entropy $(S)$ as a thermodynamic parameter,the criterion for the spontaneity of any process is

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Which of the following substances has the highest entropy?

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For the reaction $2 H_{2(g)} + O_{2(g)} \longrightarrow 2 H_2O_{(g)}$,at $300 \ K$,$\Delta G$ and $\Delta H$ of water are $-228.4 \ kJ \ mol^{-1}$ and $-241.60 \ kJ \ mol^{-1}$,respectively. Calculate the value of change in entropy for the given reaction.

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For the reactions,
$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$
$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$
What are the signs of $\Delta S$, respectively?

MediumTS EAMCET 2020

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Calculate the entropy change in the surroundings when $1.00 \ mol$ of $H_2O_{(l)}$ is formed under standard conditions. Given: $\Delta_f H^{\theta} = -286 \ kJ \ mol^{-1}$.

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Let us consider a reversible reaction at temperature,$T$. In this reaction,both $\Delta H$ and $\Delta S$ were observed to have positive values. If the equilibrium temperature is $T_e$,then the reaction becomes spontaneous at:

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Considering entropy $(S)$ as a thermodynamic parameter,the criterion for the spontaneity of any process is

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For the reaction $2 H_{2(g)} + O_{2(g)} \longrightarrow 2 H_2O_{(g)}$,at $300 \ K$,$\Delta G$ and $\Delta H$ of water are $-228.4 \ kJ \ mol^{-1}$ and $-241.60 \ kJ \ mol^{-1}$,respectively. Calculate the value of change in entropy for the given reaction.

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For the reactions,
$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$
$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$
What are the signs of $\Delta S$, respectively?