For a reaction at $25^o C$,$\Delta H > 0$ and $\Delta S > 0$. Under what conditions will this reaction become spontaneous?
- ABy increasing $T$
- BBy decreasing $T$
- CBy keeping $T$ constant
- DBy performing it in an open vessel at this temperature
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Similar Questions
For a given chemical reaction $A \rightarrow B$ at $300 \ K$,the free energy change is $-49.4 \ kJ \ mol^{-1}$ and the enthalpy of reaction is $51.4 \ kJ \ mol^{-1}$. The entropy change of the reaction is $..... \ J \ K^{-1} \ mol^{-1}$.
DifficultJEE MAIN 2021
View SolutionFor a certain reaction, $\Delta H^0 = -345 \text{ kJ}$ and $\Delta S^0 = -123 \text{ JK}^{-1}$. At what temperature will the change over from spontaneous to non-spontaneous occur (in $\text{ K}$)?
DifficultMHT CET 2026
View SolutionValues of $\Delta H$ and $\Delta S$ for five different reactions are given below. On the basis of these values,predict which one of these will be spontaneous at all temperatures.
Reaction $\Delta H \ (kJ \ mol^{-1}) / \Delta S \ (J \ K^{-1} \ mol^{-1})$ $I$ $+98.0, +14.8$ $II$ $-55.5, -84.6$ $III$ $+28.3, -17.0$ $IV$ $-40.5, +24.6$ $V$ $+34.7, 0.0$
| Reaction | $\Delta H \ (kJ \ mol^{-1}) / \Delta S \ (J \ K^{-1} \ mol^{-1})$ |
|---|---|
| $I$ | $+98.0, +14.8$ |
| $II$ | $-55.5, -84.6$ |
| $III$ | $+28.3, -17.0$ |
| $IV$ | $-40.5, +24.6$ |
| $V$ | $+34.7, 0.0$ |
Medium
View SolutionIn all spontaneous processes,which of the following is true?
Medium
View SolutionThe correct thermodynamic conditions for a spontaneous reaction at all temperatures are:
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