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Chapter 10: Problem 16

Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?

Short Answer

Expert verified
Critical temperature is the temperature above which a substance cannot be liquefied, regardless of the pressure applied, and critical pressure is the pressure required to liquefy a substance at its critical temperature. According to the kinetic molecular theory, at the critical temperature, the kinetic energy of particles becomes high enough to overcome the attractive forces between them, resulting in the substance existing solely as a gas. Therefore, it is impossible for a substance to exist as a liquid above its critical temperature.

Step by step solution

01

Definition of critical temperature

Critical temperature is the temperature above which a substance cannot be liquefied, regardless of the pressure applied. At this point, the gas phase and the liquid phase of the substance will merge into a single phase.
02

Definition of critical pressure

Critical pressure is the pressure required to liquefy a substance at its critical temperature. In other words, it is the minimum pressure required to bring about the phase transition between liquid and gas at the critical temperature.
03

Explanation using kinetic molecular theory

The kinetic molecular theory states that the properties of a substance are determined by the motion of its particles. As the temperature of a substance increases, so does the kinetic energy of its particles. This results in the particles moving faster and overcoming the attractive forces that hold them together in a liquid phase. At the critical temperature, the kinetic energy of the particles becomes high enough to completely overcome the attractive forces between them. The particles can no longer be held together as a cohesive liquid, and the substance exists solely as a gas. No matter how much pressure is applied, the substance cannot be brought back to the liquid phase, as the particles have too much energy to be confined by the attractive forces. In conclusion, by understanding the concepts of critical temperature, critical pressure, and the kinetic molecular theory, we can see why a substance cannot exist as a liquid above its critical temperature.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Critical Pressure
Understanding the concept of critical pressure is key when delving into the unique properties of substances at their boing points. It's the pressure that's required to liquefy a gas at its critical temperature. Think of it like a charm spell that has the power to turn a spirited, high-energy gas into a calm, collected liquid鈥攂ut only if the spell is strong enough.

At this critical juncture, the gas and liquid phases become indistinguishable, and they converge into a supercritical fluid. The particles within are too unruly to settle neatly into a liquid; they need just the right amount of pressure to reign them in.
Kinetic Molecular Theory
Diving into the kinetic molecular theory is a bit like peeking into the engine room of matter. In this view, particles are always on the move, jostling and zooming around. Their movement is what we feel as temperature. As this movement鈥攐r kinetic energy鈥攊ncreases, the particles want less and less to stick together. They're like teenagers yearning for freedom!

Imagine turning up the music (adding heat) and watching the dance floor (the substance) go from smooth ballroom dancing (liquid) to an energetic mosh pit (gas). Beyond a certain volume (critical temperature), no matter how much the dance floor is squeezed (pressure applied), you can't force the crowd back into a slow dance. That's the essence of why liquids can't exist above their critical temperature.
Phase Transition
The magic moment of phase transition is like the act of a skilled magician, where substances change their state from solid to liquid, liquid to gas, or vice versa. Each substance has its own signature trick, a certain combination of temperature and pressure that enables this transformation.

But at the critical temperature, the liquid state vanishes, despite our best efforts. This disappearing act is profound鈥攍ike a magician's finale鈥攍eaving us with only the gas state, no matter how much we plead or apply pressure for the liquid to return. This conclusion to a phase transition shows the ultimate power of heat and movement over attraction and cohesion among particles.

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Most popular questions from this chapter

Rationalize the difference in boiling points for each of the following pairs of substances: a. \(n\) -pentane \(\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\) \(36.2^{\circ} \mathrm{C}\) neopentane CC(C)(C)C \(9.5^{\circ} \mathrm{C}\) b. HF \(20^{\circ} \mathrm{C}\) \(\mathrm{HCl} \quad-85^{\circ} \mathrm{C}\) c. HCl \(-85^{\circ} \mathrm{C}\) \(\mathrm{LiCl} \quad 1360^{\circ} \mathrm{C}\) d. \(n\) -pentane \(\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\) \(36.2^{\circ} \mathrm{C}\) \(\begin{array}{lll}n \text { -hexane } & \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3} & 69^{\circ} \mathrm{C}\end{array}\)

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Will a crystalline solid or an amorphous solid give a simpler X-ray diffraction pattern? Why?

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