Vapor pressure in open container

In summary, the concept of vapor pressure in an open system can be difficult to understand. In an open container, equilibrium cannot be reached due to the vapor being dispersed into the atmosphere. Boiling is defined as when the vapor pressure of a liquid reaches and/or exceeds the atmospheric pressure. Bubbles form below the surface of the liquid when the vapor pressure inside the bubbles matches the atmospheric pressure. The vapor pressure in an open system cannot be measured, but it is equal to the equilibrium vapor pressure at the interface between the liquid and air. During boiling, the rate of water vapor escaping from the liquid is increased by the formation and bursting of bubbles.
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jbriggs444 said:
There is a good deal of relevant discussion in https://www.physicsforums.com/threads/negative-pressure.428998/

In that thread Andy Resnick provides a reference to http://www.nature.com/nature/journal/v278/n5700/abs/278148a0.html which discusses the tensile strength of water.
Oh yeah. I remember this thing now. I never bought into the explanation related to assuming that there is a negative pressure to get the fluid to rise in the pores above a hydrostatic column. I felt that there were some other more likely explanations, such as peristaltic pumping of the pore fluid by the walls of the pores (so that the system is not hydrostatic) or viscoelasticity of the pore fluid (beyond the "tensile strength" of water; actually tensile stiffness). Has anyone ever measured the rheological (viscoelastic) characteristics of the (biological) pore fluid in the laboratory? (Biological fluids are notoriously viscoelastic)

In any event, our excursion into the esoteric subject of the possible existence of negative absolute pressure has gone far afield of the intent of the OP's original questions. Irrespective of whether negative absolute pressure can actually exist, the formation of bubbles and the occurance of cavitation are realities that we have adequately explained in our previous responses.

Chet
 
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<h2>1. What is vapor pressure in an open container?</h2><p>Vapor pressure in an open container refers to the pressure exerted by the vapor of a substance in a container that is not completely sealed. It is a measure of the tendency of a substance to escape from its liquid or solid state and enter the gas phase.</p><h2>2. How is vapor pressure in an open container different from vapor pressure in a closed container?</h2><p>Vapor pressure in an open container is lower than vapor pressure in a closed container. This is because in an open container, some of the vapor molecules can escape into the surrounding environment, whereas in a closed container, the vapor molecules are contained and cannot escape.</p><h2>3. What factors affect the vapor pressure in an open container?</h2><p>The vapor pressure in an open container is affected by the temperature, the nature of the substance, and the surface area of the liquid in the container. Higher temperatures, more volatile substances, and larger surface areas will result in higher vapor pressures.</p><h2>4. How does vapor pressure in an open container relate to boiling point?</h2><p>Vapor pressure in an open container is directly related to the boiling point of a substance. As the vapor pressure increases, the boiling point decreases. This is because a higher vapor pressure means that more molecules are escaping from the liquid, making it easier for the substance to enter its gas phase.</p><h2>5. Why is vapor pressure in an open container important?</h2><p>Vapor pressure in an open container is important because it can affect the rate of evaporation and the stability of a substance. It is also a crucial factor in determining the boiling point of a substance. Additionally, knowledge of vapor pressure in an open container is essential for various industrial processes, such as distillation and chemical reactions.</p>

Related to Vapor pressure in open container

1. What is vapor pressure in an open container?

Vapor pressure in an open container refers to the pressure exerted by the vapor of a substance in a container that is not completely sealed. It is a measure of the tendency of a substance to escape from its liquid or solid state and enter the gas phase.

2. How is vapor pressure in an open container different from vapor pressure in a closed container?

Vapor pressure in an open container is lower than vapor pressure in a closed container. This is because in an open container, some of the vapor molecules can escape into the surrounding environment, whereas in a closed container, the vapor molecules are contained and cannot escape.

3. What factors affect the vapor pressure in an open container?

The vapor pressure in an open container is affected by the temperature, the nature of the substance, and the surface area of the liquid in the container. Higher temperatures, more volatile substances, and larger surface areas will result in higher vapor pressures.

4. How does vapor pressure in an open container relate to boiling point?

Vapor pressure in an open container is directly related to the boiling point of a substance. As the vapor pressure increases, the boiling point decreases. This is because a higher vapor pressure means that more molecules are escaping from the liquid, making it easier for the substance to enter its gas phase.

5. Why is vapor pressure in an open container important?

Vapor pressure in an open container is important because it can affect the rate of evaporation and the stability of a substance. It is also a crucial factor in determining the boiling point of a substance. Additionally, knowledge of vapor pressure in an open container is essential for various industrial processes, such as distillation and chemical reactions.

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