When solid CO2 (dry ice) is allowed to come to equilibrium in a closed constant volume container at room temperature (300K),

1. the pressure rises until it reaches 1 atm

2. the pressure rises until a liquid-gas equilibrium is reached.

3. the pressure does not change.

4. the pressure rises until a liquid-solid equilibrium is reached

2. the pressure rises until a liquid-gas equilibrium is reached.

A real life example of this is fire extinguishers which store CO2 as a liquid at room temperature at really high pressures.
Im just a student, but I think that as the dry ice sublimes into gas at low pressures, the pressure rises to a point where liquid can form. Eventually all the solid gets converted to liquid. the liquid CO2 warms to 300K and at this point an equilibrium is reached between liquid and the gas responsible for the extremely high pressures.

Marcus is right, Josie. I don't really understand it either but he is correct.

jose` is wrong

All I know is that Josie is wrong because I just do.

The answer is liquid-gas equilibrium because of the temperature. at 300K, the solid CO2 sublimates into a gas; however, in order to maintain vp, the pressure increases, condensing the gas into liquid CO2 and creating a liquid gas equilibrium. At a lower temperature (below freezing) it could be a solid-gas equilibrium. Another way to look at it is with a CO2 phase diagram

The correct answer to the question is option 3: the pressure does not change.

To understand why, let's explore the behavior of solid CO2 (dry ice) as it comes to equilibrium in a closed constant volume container at room temperature.

Dry ice sublimes, meaning it turns directly from a solid to a gas without going through the liquid phase. At room temperature and normal atmospheric pressure, dry ice sublimes around -78.5°C (-109.3°F).

In a closed constant volume container, when solid CO2 is exposed to room temperature, it will gradually sublimate into a gas. The sublimation process occurs because the vapor pressure of carbon dioxide exceeds the current pressure in the container.

As the solid CO2 sublimes, gas molecules are released and the number of gas molecules in the container increases. However, since the volume of the container remains constant, the concentration of gas molecules per unit volume also increases. This increase in concentration leads to an increase in pressure according to the ideal gas law.

However, it is important to note that the increase in pressure due to the sublimation of dry ice is counteracted by the fact that some gas molecules may condense back into solid CO2. This occurs because the sublimated CO2 gas can cool down and lose energy, leading to reformation of solid CO2.

Therefore, as the sublimation and reformation of solid CO2 occur simultaneously, the system reaches an equilibrium where the rate of sublimation equals the rate of reformation. At this equilibrium state, there is a balance between the gas molecules leaving the solid CO2 phase and the gas molecules condensing back into the solid phase.

Because the rates of sublimation and reformation are equal, the number of gas molecules in the container remains constant over time. Consequently, the concentration of gas molecules and, hence, the pressure in the container do not change.

In summary, when solid CO2 (dry ice) is allowed to come to equilibrium in a closed constant volume container at room temperature, the pressure does not change.

All I know is that Marcus is wrong because solids don't have to become liquids before they become gas. That is what is the case with dry ice. It becomes a gas before it has the time to go to a liquid.