For the reaction H_2O_{(l)} longrightarrow H_ | vedclass

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(B) The given reaction is the vaporization of water at its boiling point: $H_2O_{(l)} \longrightarrow H_2O_{(g)}$.This process occurs at equilibrium a

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$\Delta S_{	ext{system}} > 0$ & $\Delta S_{	ext{surroundings}} < 0$

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(B) The given reaction is the vaporization of water at its boiling point: $H_2O_{(l)} \longrightarrow H_2O_{(g)}$.This process occurs at equilibrium at $T=100^{\circ} C$ and $P=1 \ atm$.For any process at equilibrium,the change in entropy of the universe is zero: $\Delta S_{	ext{universe}} = \Delta S_{	ext{system}} + \Delta S_{	ext{surroundings}} = 0$.Therefore,$\Delta S_{	ext{system}} = -\Delta S_{	ext{surroundings}}$.Since vaporization involves a transition from a liquid to a gas,the disorder increases,so $\Delta S_{	ext{system}} > 0$.Consequently,$\Delta S_{	ext{surroundings}}$ must be negative,i.e.,$\Delta S_{	ext{surroundings}} < 0$.

For the reaction $H_2O_{(l)} \longrightarrow H_2O_{(g)}$ at $T=100^{\circ} C$ and $P=1 \ atm$,choose the correct option:

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