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 the reaction $PCl_5 \to PCl_3 + Cl_2$,$\Delta H = 75 \ kJ \ mol^{-1}$ and $\Delta S = 120 \ J \ K^{-1} \ mol^{-1}$. At which temperature will the reaction be spontaneous? (in $K$)
Medium
View SolutionAt the transition temperature $T$, $\Delta G^0 = 0$ and $\Delta G^0 = 105 - 35 \log T$, where $A$ and $B$ are two states of substance $X$. The transition temperature in $^\circ\text{C}$ when pressure is $1 \text{ atm}$ is . . . . . . .
DifficultJEE MAIN 2026
View SolutionIdentify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.
$A$ minus sign of the free energy change denotes that
Easy
View SolutionCalculate the value of $\Delta G$ for the following reaction at $300 \ K$.
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
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