A 0.75 L bottle is cleaned, dried, and closed in a room where the air is 24°C and 35% relative humidity (that is, the water vapor in the air is 0.35 of the equilibrium vapor pressure at 24°C). The bottle is brought outside and stored at 0.0°C. (See Table 5.2)

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3.55E-4 mol

To determine what will happen to the water content inside the bottle when it is taken outside and stored at a lower temperature, we need to consider the concept of vapor pressure and the relationship between temperature and relative humidity.

The equilibrium vapor pressure is the pressure exerted by the water vapor in a closed system when it is in equilibrium with its liquid phase. It depends on the temperature and is typically higher at higher temperatures.

In this scenario, the relative humidity inside the room is given as 35% of the equilibrium vapor pressure at 24°C. This means that the actual pressure of the water vapor in the room is 0.35 times the equilibrium vapor pressure at 24°C.

The bottle is then taken outside and stored at 0.0°C, which is a lower temperature compared to the room temperature. Lowering the temperature generally reduces the equilibrium vapor pressure since colder air has a lower capacity to hold water vapor.

To determine what happens to the water content inside the bottle, we can compare the actual vapor pressure inside the bottle at 24°C with the equilibrium vapor pressure at 0°C.

First, we need to calculate the actual vapor pressure inside the bottle at 24°C. To do this, we determine 0.35 times the equilibrium vapor pressure at 24°C.

Next, we need to find the equilibrium vapor pressure at 0°C using a table or vapor pressure calculator. This value represents the maximum amount of water vapor that the air at 0°C can hold.

Comparing these two values will give us an idea of whether the water vapor inside the bottle will condense or not.

Using Table 5.2 or a vapor pressure calculator, find the equilibrium vapor pressure at 0°C.

Finally, compare the actual vapor pressure inside the bottle at 24°C with the equilibrium vapor pressure at 0°C:

- If the actual vapor pressure inside the bottle at 24°C is lower than the equilibrium vapor pressure at 0°C, the water vapor inside the bottle will condense, resulting in liquid water forming inside the bottle.
- If the actual vapor pressure inside the bottle at 24°C is higher than the equilibrium vapor pressure at 0°C, the water vapor inside the bottle will not condense, and the water content will remain in the vapor phase.

By following this process, you can determine what will happen to the water content inside the bottle when it is taken outside and stored at a lower temperature.