For the change $H_2O_{(l)} \to H_2O_{(g)}$ at $P = 1 \ atm$ and $T = 373 \ K$,the free energy change $\Delta G = 0$. This indicates that:
- A$H_2O_{(l)}$ is in equilibrium with $H_2O_{(g)}$
- BWater boils spontaneously at $373 \ K$
- CWater does not boil spontaneously at $373 \ K$
- DCondensation of water vapour occurs spontaneously at $373 \ K$
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Similar Questions
For 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 SolutionWhich of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?
The entropy and enthalpy changes for the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ at $300 \ K$ and $1 \ atm$ are respectively $-42.4 \ J \ K^{-1}$ and $-41.2 \ kJ$. The temperature at which the reaction will go in the reverse direction is (in $K$)
At a temperature of $25^\circ C$,if $\Delta H < T \Delta S$,then $\Delta G$ = ?
Easy
View SolutionCompare the following criteria for spontaneity of a reaction based on the values of $\Delta_{\text{r}}H^0$,$\Delta_{\text{r}}S^0$,and $\Delta_{\text{r}}G^0$:
$\Delta_{\text{r}}H^0$ $\Delta_{\text{r}}S^0$ $\Delta_{\text{r}}G^0$ Description $(a) (+)$ $(-)$ $(+)$ $(i) \text{ Non-spontaneous at all temperatures}$ $(b) (-)$ $(-)$ $(-)$ $(ii) \text{ Spontaneous at low temperatures}$ $(c) (-)$ $(+)$ $(-)$ $(iii) \text{ Spontaneous at all temperatures}$
| $\Delta_{\text{r}}H^0$ | $\Delta_{\text{r}}S^0$ | $\Delta_{\text{r}}G^0$ | Description |
|---|---|---|---|
| $(a) (+)$ | $(-)$ | $(+)$ | $(i) \text{ Non-spontaneous at all temperatures}$ |
| $(b) (-)$ | $(-)$ | $(-)$ | $(ii) \text{ Spontaneous at low temperatures}$ |
| $(c) (-)$ | $(+)$ | $(-)$ | $(iii) \text{ Spontaneous at all temperatures}$ |
Medium
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