05. Gibbs Energy Change and Equilibrium
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Thermodynamics

273090 $\begin{aligned}
& \mathrm{PbO}_2 \rightarrow \mathrm{PbO}, \Delta \mathrm{G}_{298}<0 \\
& \mathrm{SnO}_2 \rightarrow \mathrm{SnO}, \Delta \mathrm{G}_{298}>0
\end{aligned}$
Most probable oxidation state of $\mathrm{Pb}$ and $\mathrm{Sn}$ will be

1 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{4+}$
2 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{2+}$
3 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{2+}$
4 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{4+}$
NEET-2001
Thermodynamics

273092 For vaporization of water at 1 atmospheric pressure, the values of $\Delta H$ and $\Delta S$ are $40.63 \mathrm{~kJ}$ mol $^{-1}$ and $108.8 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, respectively. The temperature when Gibbs' energy change $(\Delta \mathbf{G})$ for this transformation will be zero, is

1 $273.4 \mathrm{~K}$
2 $393.4 \mathrm{~K}$
3 $373.4 \mathrm{~K}$
4 $293.4 \mathrm{~K}$
NEET-2010
Thermodynamics

273093 For the reaction, $\mathrm{X}_2 \mathrm{O}_4(l) \rightarrow 2 \mathrm{XO}_2(\mathrm{~g})$ $\Delta \mathrm{U}=2.1$ kcal, $\Delta \mathrm{S}=20$ cal $\mathrm{K}^{-1}$ at $300 \mathrm{~K}$ hence, $\Delta \mathbf{G}$ is

1 $2.7 \mathrm{kcal}$
2 $-2.7 \mathrm{kcal}$
3 $9.3 \mathrm{kcal}$
4 $-9.3 \mathrm{kcal}$
NEET-2014
Thermodynamics

273094 A reaction having equal energies of activation for forward and reverse reactions has

1 $\Delta \mathrm{H}=0$
2 $\Delta \mathrm{H}=\Delta \mathrm{G}=\Delta \mathrm{S}=0$
3 $\Delta \mathrm{S}=0$
4 $\Delta \mathrm{G}=0$
NEET 2013
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Thermodynamics

273090 $\begin{aligned}
& \mathrm{PbO}_2 \rightarrow \mathrm{PbO}, \Delta \mathrm{G}_{298}<0 \\
& \mathrm{SnO}_2 \rightarrow \mathrm{SnO}, \Delta \mathrm{G}_{298}>0
\end{aligned}$
Most probable oxidation state of $\mathrm{Pb}$ and $\mathrm{Sn}$ will be

1 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{4+}$
2 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{2+}$
3 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{2+}$
4 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{4+}$
NEET-2001
Thermodynamics

273092 For vaporization of water at 1 atmospheric pressure, the values of $\Delta H$ and $\Delta S$ are $40.63 \mathrm{~kJ}$ mol $^{-1}$ and $108.8 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, respectively. The temperature when Gibbs' energy change $(\Delta \mathbf{G})$ for this transformation will be zero, is

1 $273.4 \mathrm{~K}$
2 $393.4 \mathrm{~K}$
3 $373.4 \mathrm{~K}$
4 $293.4 \mathrm{~K}$
NEET-2010
Thermodynamics

273093 For the reaction, $\mathrm{X}_2 \mathrm{O}_4(l) \rightarrow 2 \mathrm{XO}_2(\mathrm{~g})$ $\Delta \mathrm{U}=2.1$ kcal, $\Delta \mathrm{S}=20$ cal $\mathrm{K}^{-1}$ at $300 \mathrm{~K}$ hence, $\Delta \mathbf{G}$ is

1 $2.7 \mathrm{kcal}$
2 $-2.7 \mathrm{kcal}$
3 $9.3 \mathrm{kcal}$
4 $-9.3 \mathrm{kcal}$
NEET-2014
Thermodynamics

273094 A reaction having equal energies of activation for forward and reverse reactions has

1 $\Delta \mathrm{H}=0$
2 $\Delta \mathrm{H}=\Delta \mathrm{G}=\Delta \mathrm{S}=0$
3 $\Delta \mathrm{S}=0$
4 $\Delta \mathrm{G}=0$
NEET 2013
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Thermodynamics

273090 $\begin{aligned}
& \mathrm{PbO}_2 \rightarrow \mathrm{PbO}, \Delta \mathrm{G}_{298}<0 \\
& \mathrm{SnO}_2 \rightarrow \mathrm{SnO}, \Delta \mathrm{G}_{298}>0
\end{aligned}$
Most probable oxidation state of $\mathrm{Pb}$ and $\mathrm{Sn}$ will be

1 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{4+}$
2 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{2+}$
3 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{2+}$
4 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{4+}$
NEET-2001
Thermodynamics

273092 For vaporization of water at 1 atmospheric pressure, the values of $\Delta H$ and $\Delta S$ are $40.63 \mathrm{~kJ}$ mol $^{-1}$ and $108.8 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, respectively. The temperature when Gibbs' energy change $(\Delta \mathbf{G})$ for this transformation will be zero, is

1 $273.4 \mathrm{~K}$
2 $393.4 \mathrm{~K}$
3 $373.4 \mathrm{~K}$
4 $293.4 \mathrm{~K}$
NEET-2010
Thermodynamics

273093 For the reaction, $\mathrm{X}_2 \mathrm{O}_4(l) \rightarrow 2 \mathrm{XO}_2(\mathrm{~g})$ $\Delta \mathrm{U}=2.1$ kcal, $\Delta \mathrm{S}=20$ cal $\mathrm{K}^{-1}$ at $300 \mathrm{~K}$ hence, $\Delta \mathbf{G}$ is

1 $2.7 \mathrm{kcal}$
2 $-2.7 \mathrm{kcal}$
3 $9.3 \mathrm{kcal}$
4 $-9.3 \mathrm{kcal}$
NEET-2014
Thermodynamics

273094 A reaction having equal energies of activation for forward and reverse reactions has

1 $\Delta \mathrm{H}=0$
2 $\Delta \mathrm{H}=\Delta \mathrm{G}=\Delta \mathrm{S}=0$
3 $\Delta \mathrm{S}=0$
4 $\Delta \mathrm{G}=0$
NEET 2013
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Thermodynamics

273090 $\begin{aligned}
& \mathrm{PbO}_2 \rightarrow \mathrm{PbO}, \Delta \mathrm{G}_{298}<0 \\
& \mathrm{SnO}_2 \rightarrow \mathrm{SnO}, \Delta \mathrm{G}_{298}>0
\end{aligned}$
Most probable oxidation state of $\mathrm{Pb}$ and $\mathrm{Sn}$ will be

1 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{4+}$
2 $\mathrm{Pb}^{4+}, \mathrm{Sn}^{2+}$
3 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{2+}$
4 $\mathrm{Pb}^{2+}, \mathrm{Sn}^{4+}$
NEET-2001
Thermodynamics

273092 For vaporization of water at 1 atmospheric pressure, the values of $\Delta H$ and $\Delta S$ are $40.63 \mathrm{~kJ}$ mol $^{-1}$ and $108.8 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, respectively. The temperature when Gibbs' energy change $(\Delta \mathbf{G})$ for this transformation will be zero, is

1 $273.4 \mathrm{~K}$
2 $393.4 \mathrm{~K}$
3 $373.4 \mathrm{~K}$
4 $293.4 \mathrm{~K}$
NEET-2010
Thermodynamics

273093 For the reaction, $\mathrm{X}_2 \mathrm{O}_4(l) \rightarrow 2 \mathrm{XO}_2(\mathrm{~g})$ $\Delta \mathrm{U}=2.1$ kcal, $\Delta \mathrm{S}=20$ cal $\mathrm{K}^{-1}$ at $300 \mathrm{~K}$ hence, $\Delta \mathbf{G}$ is

1 $2.7 \mathrm{kcal}$
2 $-2.7 \mathrm{kcal}$
3 $9.3 \mathrm{kcal}$
4 $-9.3 \mathrm{kcal}$
NEET-2014
Thermodynamics

273094 A reaction having equal energies of activation for forward and reverse reactions has

1 $\Delta \mathrm{H}=0$
2 $\Delta \mathrm{H}=\Delta \mathrm{G}=\Delta \mathrm{S}=0$
3 $\Delta \mathrm{S}=0$
4 $\Delta \mathrm{G}=0$
NEET 2013