what happens to water at 100 degrees celsius as pressure is increased fro 0.8 atm to 1.2 atm?
It goes from the gas phase to liquid phase. Water vapor to liquid water. - apex
When the pressure is increased from 0.8 atm to 1.2 atm, the boiling point of water also increases. In normal conditions, water boils at 100 degrees Celsius at 1 atmosphere of pressure (1 atm). However, when pressure is increased, the boiling point of water also increases.
At 1.2 atm, the boiling point of water will be slightly higher than 100 degrees Celsius. This means that water will remain in its liquid state at that temperature and pressure, instead of boiling and turning into vapor.
So, at 100 degrees Celsius and 1.2 atm pressure, water would still be in liquid form.
To understand what happens to water at different pressures and temperatures, it's important to look at the phase diagram of water. A phase diagram shows the relationship between temperature, pressure, and the physical state of a substance.
In the case of water, at normal atmospheric pressure (1 atm), it boils at 100 degrees Celsius and becomes a gas. As pressure increases, the boiling point of water also increases.
If we start with water at 0.8 atm and increase the pressure to 1.2 atm while keeping the temperature at 100 degrees Celsius, we can consult the phase diagram to determine the outcome.
At 100 degrees Celsius and 0.8 atm, according to the phase diagram, water is already in its gaseous state. Therefore, further increasing the pressure to 1.2 atm will not cause any significant change. The water will remain in the gas phase.
However, it's important to note that if the temperature were lower than 100 degrees Celsius, increasing the pressure could potentially cause the water to transition from a gas back into a liquid state.