Which of the following conditions indicates the reaction is spontaneous?
- A$\Delta S < 0, \Delta H > 0, \Delta G > 0$ at all temperatures
- B$\Delta S < 0, \Delta H > 0, \Delta G > 0$ at low temperatures
- C$\Delta S > 0, \Delta H < 0, \Delta G < 0$ at all temperatures
- D$\Delta S < 0, \Delta H > 0, \Delta G > 0$ at high temperatures
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Similar Questions
For a spontaneous process, the incorrect statement is
Based on the provided table, which of the following options correctly identifies the spontaneous reactions?
$\Delta_r H^{\circ}$ $\Delta_r S^{\circ}$ $\Delta_r G^{\circ}$ Spontaneity of the reaction $A$ $+$ $+$ $+$ Spontaneous at low $T$ $B$ $+$ $+$ $-$ Spontaneous at high $T$ $C$ $-$ $-$ $-$ Spontaneous at low $T$ $D$ $+$ $-$ $+$ Spontaneous at high $T$
| $\Delta_r H^{\circ}$ | $\Delta_r S^{\circ}$ | $\Delta_r G^{\circ}$ | Spontaneity of the reaction | |
|---|---|---|---|---|
| $A$ | $+$ | $+$ | $+$ | Spontaneous at low $T$ |
| $B$ | $+$ | $+$ | $-$ | Spontaneous at high $T$ |
| $C$ | $-$ | $-$ | $-$ | Spontaneous at low $T$ |
| $D$ | $+$ | $-$ | $+$ | Spontaneous at high $T$ |
Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.
Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?
MediumAIPMT 2005
View SolutionThe densities of graphite and diamond at $298 \, K$ are $2.25 \, g \, cm^{-3}$ and $3.31 \, g \, cm^{-3}$ respectively. If the standard free energy difference $(\Delta G^o)$ is $1895 \, J \, mol^{-1}$, the pressure at which graphite will be transformed into diamond at $298 \, K$ is:
MediumAIPMT 2003
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