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Chapter 11: Problem 146

Describe how you would adjust the temperature and pressure of a gas to convert it to the liquid state.

Short Answer

Expert verified
Lower the temperature and/or increase the pressure of the gas.

Step by step solution

01

Understanding the Basics

To convert a gas to a liquid, we must move the gas through its phase diagram to reach conditions where it is in the liquid state, typically involving lowering the temperature or increasing the pressure.
02

Lowering Temperature

One way to convert a gas into a liquid is by lowering its temperature. When the temperature decreases, the kinetic energy of the gas molecules reduces, allowing intermolecular forces to draw the molecules closer together to form a liquid.
03

Increasing Pressure

Another method is by increasing pressure. By applying more pressure to the gas, the molecules are forced closer together. This increase in pressure can cause the gas to condense into a liquid even if the temperature remains constant.
04

Adjusting Both Temperature and Pressure

In many cases, a combination of both lowering the temperature and increasing the pressure is used. This ensures that the gas transitions smoothly to a liquid state, as both conditions synergistically help overcome kinetic energy that keeps the molecules apart.

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Key Concepts

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

Temperature Reduction
When we talk about reducing the temperature of a gas, we mean that we are lowering the average kinetic energy of its molecules. The kinetic energy of gas molecules is responsible for keeping them apart from one another, maintained in a gaseous form. As the temperature drops:
  • The molecules slow down in movement, giving less energy to resist attractive forces.
  • The reduced movement allows molecules to experience more intermolecular forces, drawing them closer together.
This reduced distance lets the gas naturally shift into a liquid state. Practically speaking, this could involve using refrigeration techniques or simply reducing the thermal energy imparted to the gas system. Remember, lower temperatures mean molecules are more leisurely, creating a conducive environment for phase transition from gas to liquid.
Pressure Increase
Pressure plays a significant role in shifting gas to a liquid. By increasing the pressure exerted on a gas, we compress its molecules closer together without necessarily changing the temperature. Here's what happens:
  • More pressure means fewer spaces between the gas molecules.
  • Compression leads to increased opportunities for intermolecular attractions.
  • Even if the gas is initially at a higher temperature, enough pressure will encourage condensation.
In industrial settings and natural environments, pressure can be manipulated through mechanical compression or changes in the gas container's volume to facilitate phase transitions. This property makes pressure a powerful tool alongside temperature changes in phase diagrams.
Phase Diagram
A phase diagram is like a road map for understanding how and when a substance changes its state based on temperature and pressure conditions. These diagrams provide an overview of:
  • Various states (solid, liquid, gas) and where they occur about specific temp-pressure points.
  • The boundaries between phases, known as phase boundaries.
  • Critical and triple points, representing conditions of simultaneous phase existence.
To navigate a phase diagram effectively:
Identify the current state of the substance and the axis indicating its pressure and temperature.
Move toward the liquid phase by reducing temperature, increasing pressure, or both, as needed. Understanding phase diagrams allows one to predict and create conditions for phase transitions, facilitating practical applications in chemistry and engineering.

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Most popular questions from this chapter

Barium metal has a body-centered cubic lattice with all atoms at lattice points; its density is \(3.51 \mathrm{~g} / \mathrm{cm}^{3} .\) From these data and the atomic weight, calculate the edge length of a unit cell.

On the basis of the description given, classify each of the following solids as molecular, metallic, ionic, or covalent network. Explain your answers. a lustrous, yellow solid that conducts electricity b) a hard, black solid melting at \(2350^{\circ} \mathrm{C}\) to give a nonconducting liquid c a nonconducting, pink solid melting at \(650^{\circ} \mathrm{C}\) to give an electrically conducting liquid d. red crystals having a characteristic odor and melting at \(171^{\circ} \mathrm{C}\)

Explain why evaporation leads to cooling of the liquid.

Under the right conditions, hydrogen gas, \(\mathrm{H}_{2}\), can be liquefied. Which is the most important intermolecular force that is responsible for allowing hydrogen molecules to be liquefied? hydrogen bonding dipole-dipole interactions London (dispersion) forces covalent bonds ion-dipole forces

The vapor pressure of a volatile liquid can be determined by slowly bubbling a known volume of gas through the liquid at a given temperature and pressure. In an experiment, a 5.40-L sample of nitrogen gas, \(\mathrm{N}_{2}\), at \(20.0^{\circ} \mathrm{C}\) and \(745 \mathrm{mmHg}\) is bubbled through liquid isopropyl alcohol, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O},\) at \(20.0^{\circ} \mathrm{C}\). Nitrogen containing the vapor of \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\) at its vapor pressure leaves the vessel at \(20.0^{\circ} \mathrm{C}\) and \(745 \mathrm{mmHg} .\) It is found that \(0.6149 \mathrm{~g} \mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\) has evapo- rated. How many moles of \(\mathrm{N}_{2}\) are in the gas leaving the liquid? How many moles of alcohol are in this gaseous mixture? What is the mole fraction of alcohol vapor in the gaseous mixture? What is the partial pressure of the alcohol in the gaseous mixture? What is the vapor pressure of \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\) at \(20.0^{\circ} \mathrm{C} ?\)
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