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Chapter 11: Problem 102

The liquid-vapor boundary line in the phase diagram of any substance always stops abruptly at a certain point. Why?

Short Answer

Expert verified
The liquid-vapor boundary line in a phase diagram ends abruptly at the critical point. This is the highest temperature and pressure at which the liquid and gas phases of a substance can co-exist. Beyond this point, the substance exists as a supercritical fluid, exhibiting properties of both gas and liquid.

Step by step solution

01

Defining a phase diagram

A phase diagram is a graphical representation of the physical states of a substance under different temperatures and pressures. It shows when a substance exists in solid, liquid, or gas form, and indicates where transitions between these states occur.
02

Understanding liquid-vapor boundary line

The liquid-vapor boundary line in a phase diagram separates the temperature and pressure conditions under which the substance exists as a liquid from those in which it exists as a gas or vapor. Along this line, the substance can freely transition between these two states.
03

Explaining the abrupt stop of the liquid-vapor line

The abrupt end of the liquid-vapor boundary line at a certain point is called the critical point. This is the highest temperature and pressure at which liquid and gas phases of a substance can co-exist. Beyond the critical point, there is no distinction between the liquid and gas phases, and the substance exists as a supercritical fluid, which can diffuse through solids like a gas, and dissolve compounds like a liquid.

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Most popular questions from this chapter

Gaseous or highly volatile liquid anesthetics are often preferred in surgical procedures because once inhaled, these vapors can quickly enter the bloodstream through the alveoli and then enter the brain. Shown here are several common gaseous anesthetics with their boiling points. Based on intermolecular force considerations, explain the advantages of using these anesthetics. (Hint: The brain barrier is made of membranes that have a nonpolar interior region.)

A flask of water is connected to a powerful vacuum pump. When the pump is turned on, the water begins to boil. After a few minutes, the same water begins to freeze. Eventually, the ice disappears. Explain what happens at each step.

At \(-35^{\circ} \mathrm{C}\), liquid \(\mathrm{HI}\) has a higher vapor pressure than liquid HF. Explain.

How is the rate of evaporation of a liquid affected by (a) temperature, (b) the surface area of a liquid exposed to air, (c) intermolecular forces?

The vapor pressure of liquid \(X\) is lower than that of liquid \(Y\) at \(20^{\circ} \mathrm{C},\) but higher at \(60^{\circ} \mathrm{C}\). What can you deduce about the relative magnitude of the molar heats of vaporization of \(\mathrm{X}\) and \(\mathrm{Y} ?\)
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