A glass initially contains 0.1 kg of ice and 0.05 kg of water. The ice, the water, the glass and the air surrounding them are all at T = 273.15 K and P = 0.1 MPa. The water is evaporating very gradually. Which of the following is true?
A. The ice and water are at equilibrium with each other and with the surroundings.
B. The ice and water are not in equilibrium with each other, but if 0.025 kg of ice melted, making the masses of the ice and water equal, they would then be in equilibrium with each other.
C. The water is in thermal and mechanical equilibrium with the air, but not in chemical equilibrium.
D. The system is at steady state but not in equilibrium.
E. None of the above are true.
A. Incorrect. If the water was at equilibrium with its surroundings, it would not be evaporating at all. Try again.
B. Incorrect. There is no reason why phases in equilibrium need to have the same mass. If no water is freezing and no ice is melting, then the water and ice are in chemical equilibrium with each other regardless of the masses of the phases.
C. Correct. The water and air are at the same temperature and pressure, but they are not in chemical equilibrium; there is a driving force for water to evaporate. In practical terms, the air is not fully saturated with water vapor (relative humidity is less than 100%). Vapor–liquid equilibrium is addressed for pure components in Chapter 8 and for multi-component mixtures in Chapters 12 and 13.
D. Incorrect. Because water is evaporating from the glass and not being replenished from any source, we cannot say it is at steady state. Try again.
E. Incorrect. One of the statements is correct. Try again.
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