What is phase equilibrium? What are some examples?
I would expand upon the other postings with this:A substance is in “phase equilbrium” when more than one phase of a substance (solid, liquid, gas) is present *and* the amount of material in each phase does not change.Water is a good example because it happens in real life and is easy to understand. Imagine the co-existence of solid and vapor forms of water in a freezer (without auto-defrost) compartment that hasn’t been opened in a while. In a closed contain of water, the vapor and liquid phases quickly come to equibrium as long as the temperature and air pressure are constant.There is a “triple” point for water in which ice, liquid, and vapor can all be present: Triple point - Wikipedia. This is a specific temperature and pressure. The Wikipedia article describes this point for water, mercury, carbon dioxide, and many more.Note also that the cool phase diagram there has lines between the phases. These are points of phase equilibrium (temperature and pressure). And, even more exciting, it shows that the various phases of ice (yes, there are multiple forms) are stable under different conditions. Pressure matters a lot!Equilibrium does not mean, however, that there is no change. Equilbrium is dynamic. In the freezer, some of the ice will sublime and some of the vapor will condense to the solid form, giving the “frost” on the sides of the freezer.In the closed container, water is continually evaporating and condensing, but we can only see it in the beads of water or condensation that may appear one along the insides of the container.One more cool fact about the diagram: the “critical point” at the right shows the temperature and pressure where the liquid and vapor phases are “merged”. At that place, one can think of a very think gas or a very vaporous liquid. There’s no difference in this hot, high pressure condition.
On a phase diagram, the critical temperature is __________.?
On a phase diagram, the critical temperature is __________. A) the temperature at which all three states are in equilibrium B) the temperature required to cause sublimation of a solid C) the temperature above which a gas cannot be liquefied D) the temperature required to melt a solid E) the temperature below which a gas cannot be liquefied
How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a phase d?
The correct answer is a) by a line separating the phases. Each point on the line represents a combination of P and T where both phases can exist. The regions between lines are the single phase regions, where only one phase is stable. The triple point represents three phase coexistence, whereas the question only asks about 2 phases. If you're confused, just think about water: If the temperature is above freezing (and you assume standard atmospheric pressure), liquid water is stable, so ice will melt. If below freezing, water will freeze. But, if you are right at the freezing point, water and ice can both be in equilibrium. This means that you are at one of the points on the line between liquid water and ice.
Test Tmrw! At a pressure of 1 atmosphere, what is the temperature of a mixture of stream & water @ equilibrium?
100 C. What you're missing is that when you've got a mixture of two phases, that means that you're going through a phase change. At a phase change, the temperature holds constant. So, the temperature of a mixture of steam and water at 1 atm is the boiling point of water at 1 atm.
The temperature at which the solid and liquid phases of matter exist in equilibrium is called its?
The temperature at which the solid and liquid phases of matter exist in equilibrium is called its 1. melting point 2. boiling point 3. heat of fusion 4. heat of vaporization
What do each of the solid lines on a phase diagram represent?
What do each of the solid lines on a phase diagram represent? a) If a line has a positive slope, that means that the solid is more dense than the liquid, because as temperature increases so does pressure. b) The lines represent where the critical point occurs in a phase diagram. c) Each line represents the amount of energy needed to convert one phase to another at a specific temperature. d) Each line is a continuous set of temperature and pressure values where two phases of a substance are in equilibrium.