(B) For any spontaneous (irreversible) process in an isolated system,the change in entropy is positive,i.e.,$(dS)_{V,E} > 0$.For a process occurring a

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$(dS)_{V,E} > 0, (dG)_{T,P} < 0$

(B) For any spontaneous (irreversible) process in an isolated system,the change in entropy is positive,i.e.,$(dS)_{V,E} > 0$.For a process occurring at constant temperature $(T)$ and pressure $(P)$ involving only pressure-volume work,the spontaneity criterion is given by the change in Gibbs free energy,which must be negative,i.e.,$(dG)_{T,P} Therefore,the correct criteria are $(dS)_{V,E} > 0$ and $(dG)_{T,P} < 0$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

In an irreversible process taking place at constant $T$ and $P$ and in which only pressure-volume work is being done,the change in Gibbs free energy $(dG)$ and change in entropy $(dS)$ satisfy the criteria:

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A
$(dS)_{V,E} < 0, (dG)_{T,P} < 0$
B
$(dS)_{V,E} > 0, (dG)_{T,P} < 0$
C
$(dS)_{V,E} = 0, (dG)_{T,P} = 0$
D
$(dS)_{V,E} = 0, (dG)_{T,P} > 0$

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In an irreversible process taking place at constant $T$ and $P$ and in which only pressure-volume work is being done,the change in Gibbs free energy $(dG)$ and change in entropy $(dS)$ satisfy the criteria:

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Calculate the difference between $\Delta H$ and $\Delta U$ for the following reaction at $25^{\circ} C$:$C_2H_{6(g)} + 3.5O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$(Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$) (in $kJ$)

The heat of vaporisation and heat of fusion of $H_2O$ are $540 \, cal/g$ and $80 \, cal/g$. The ratio of $\frac{\Delta S_{vap}}{\Delta S_{fusion}}$ for water is :-

One mole of $CH_3OH$ is vaporized at $338 \ K$ and $1.5 \ atm$ pressure. If the enthalpy of vaporization of $CH_3OH$ is $35.57 \ kJ/mol$,calculate the value of $\Delta U$ for the process in $kJ$. (in $.76$)

Calculate the difference between heat of combustion of carbon monoxide gas at constant pressure and at constant volume at $27^{\circ} C$ (in $cal$)? $(R = 2 \ cal \ K^{-1} \ mol^{-1})$

For the reactions,$C + O_2 \to CO_2; \Delta H = -393 \ J$ $2Zn + O_2 \to 2ZnO; \Delta H = -412 \ J$

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Calculate the difference between $\Delta H$ and $\Delta U$ for the following reaction at $25^{\circ} C$:
$C_2H_{6(g)} + 3.5O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$
(Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$) (in $kJ$)

For the reactions,$C + O_2 \to CO_2; \Delta H = -393 \ J$
$2Zn + O_2 \to 2ZnO; \Delta H = -412 \ J$