Question

silid carbon dioxide sublimise at room temperature​

Answer 1

Hy here is your Ans....

• The temperature of the Earth is also too warm for carbon dioxide to be stable as a solid, so it vaporizes. The process is very similar to boiling, except that the atmospheric pressure is too low to allow carbon dioxide to become a liquid, so it "boils" directly from solid to gas.

Answer 2

Answer:

Great question!

The process of phase transitions depends largely on the material properties of the molecule. Intermolecular forces (bonds) play a large role in determining when and how a substance changes phases. Generally, the phase depends on two factors: temperature and pressure.

Plotting the phases on a graph with these two factors as axes is called a [pressure-temperature] phase diagram. Most compounds show three phases when cooling at a constant, room pressure (i.e. water), but sometimes compounds like carbon dioxide skip the liquid phase altogether and transition directly to a solid when cooled. This is because the pressure at normal atmosphere is too low for carbon dioxide to condense to a liquid. However, we can isolate the gas in a high-pressure vessel and then cool it to exhibit a liquid phase. Nevertheless, many materials can exhibit wildly different phase behaviors. For instance, if you had water at high pressure and at 0 degrees Celsius and decreased the pressure, the order of phases would be liquid -> solid -> vapor!