What is the value of $\Delta G$ for a water system in an environment at a temperature of $100 \ K$?
(C) The freezing point of water is $273 \ K$ at $1 \ \text{atm}$ pressure.
At $100 \ K$,the system is below the freezing point of water.
Since the temperature is below the phase transition temperature $(273 \ K)$,the process of freezing (liquid to solid) is spontaneous.
For a spontaneous process,the change in Gibbs free energy is negative,i.e.,$\Delta G < 0$.
At $100 \ K$,the system is below the freezing point of water.
Since the temperature is below the phase transition temperature $(273 \ K)$,the process of freezing (liquid to solid) is spontaneous.
For a spontaneous process,the change in Gibbs free energy is negative,i.e.,$\Delta G < 0$.
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Similar Questions
Values 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 | $\Delta H \ (kJ \ mol^{-1}) / \Delta S \ (J \ K^{-1} \ mol^{-1})$ |
|---|---|
| $I$ | $+98.0, +14.8$ |
| $II$ | $-55.5, -84.6$ |
| $III$ | $+28.3, -17.0$ |
| $IV$ | $-40.5, +24.6$ |
| $V$ | $+34.7, 0.0$ |
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