Name: liquid-gas changes on pv curves
Uploaded: 2025-05-22T09:05:49.000Z
Duration: 1 min 18 s
Channel: JoVE

K12 Standards

Tennessee Academic Standards

High School

Chemistry

Matter and Its Interactions

CHEM1.PS1.6

pV-Diagrams

Para un gas ideal, la presión por el volumen es una constante si la temperatura y el número de moles son constantes. El gráfico de presión frente a volumen da como resultado una hipérbola llamada isoterma pV. Para diferentes temperaturas constantes, se traza el conjunto de diagramas pV.
Los gases no ideales se comportan como un gas ideal a temperaturas más altas. Si la temperatura de un gas no ideal se reduce a una temperatura crítica, la curva pV muestra una región con pendientes cero.
Supongamos que la temperatura se baja aún más, la región que tiene pendiente cero aumenta. Estas regiones representan un cambio en el volumen sin ningún cambio en la presión.
Para la isoterma T2, la región A-B de la isoterma representa la fase de licuación. El gas se encuentra en estado de vapor hasta el punto A y en fase líquida más allá del punto B.
Para isotermas con temperaturas inferiores a T2, la licuación comienza a presiones más bajas y volúmenes más altos.
En el caso de las isotermas por encima de las temperaturas críticas, no se produce licuación. La temperatura crítica es una propiedad del gas bajo estudio para una presión crítica dada.

<ol>
	<li>Young, H.D y Freedman, R.A. (2012). Física Universitaria con Física Moderna. San Francisco, CA: Pearson; Sección 18.1; Página 596.</li>
	<li>OpenStax. (2019). Física Universitaria Vol. 2. [Versión web]. Obtenido de <a href="https://openstax.org/details/books/university-physics-volume-2">https://openstax.org/details/books/university-physics-volume-2</a>; Sección 2.1; página 75 -77.</li>
</ol>

diagramas de pv

El diagrama de pV, que es un gráfico de presión versus volumen del gas en estudio, es útil para describir ciertos aspectos de la sustancia. Cuando la sustancia se comporta como un gas ideal, la ecuación del gas ideal describe la relación entre su presión y volumen. En un diagrama de pV, es común trazar una isotermia, que es una curva que muestra p como función de V con el número de moléculas y la temperatura fija. Luego, para un gas ideal, el producto de la presión del gas y su volumen es constante. Por ejemplo, el volumen del gas disminuye a medida que aumenta la presión. El gráfico pV resultante es una hipérbola.

 Las isotermas de pV son hiperbólicas a altas temperaturas y bajas presiones. A medida que enfriamos el gas, el gráfico pV se desvía de la hipérbola. En una temperatura crítica (Tc), la curva pV muestra un punto con una pendiente cero. A medida que el gas se enfría aún más, la curva pV comienza a mostrar una región de pendiente cero. Dentro de esta región, el volumen del gas cambia, pero eso no cambia su presión. Este comportamiento corresponde a la ebullición y la condensación; cuando una sustancia está a su temperatura de ebullición para una presión determinada, puede aumentar su volumen a medida que parte del líquido se convierte en gas (pasando de un volumen más bajo a uno más alto) o disminuir a medida que parte del gas se convierte en líquido (pasando de un volumen más alto a uno más bajo), sin ningún cambio en la temperatura o presión. Esta es la región donde tiene lugar la vaporización o la licuefacción.
 <img alt="Figure1" src="/files/ftp_upload/13669/13669_PT_Figure.svg" style="text-align: center; height: 250px;"> 

 Las partes más empinadas de las curvas a la izquierda de la región de transición muestran la fase líquida, que es casi incompresible: una ligera disminución en el volumen requiere un aumento significativo en la presión. Las partes planas muestran la transición líquido-gas, representando combinaciones de presión y volumen donde el líquido y el gas pueden coexistir. A la derecha de la región de transición se muestra la fase gaseosa.

 Las isotermas por encima de Tc no pasan por la transición líquido-gas. Por lo tanto, el líquido no puede existir por encima de esa temperatura, la temperatura crítica. A una presión suficientemente baja por encima de esa temperatura, el gas tiene la densidad de un líquido pero no se condensará; se dice que el gas está en estado supercrítico. A una presión más alta, se convierte en sólido. Por ejemplo, el dióxido de carbono no tiene fase líquida a una temperatura superior a 31 grados Celsius. La presión crítica es la presión máxima a la que el líquido puede existir. El punto en el diagrama pV en la presión y temperatura críticas es el punto crítico.

Diagramas de pV

El diagrama pV, que es un gráfico de presión frente a volumen del gas en estudio, es útil para describir ciertos aspectos de la sustancia. Cuando el ...

Education

Educación

JoVE Core

Physics

Física

Unit 1

Unidad 1

The Kinetic Theory of Gases

La teoría cinética de los gases

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

liquid-gas changes on pv curves

pV curves show how gas pressure changes with volume. A pV diagram is a graph of pressure versus volume for the gas being studied. It helps describe how the substance behaves. When the gas acts like an ideal gas, the ideal gas equation gives the link between pressure and volume.

A common pV curve is an isotherm, which is a line drawn at fixed temperature and fixed number of molecules. For an ideal gas, pressure times volume stays constant. That means volume goes down as pressure goes up. The curve is a hyperbola, especially at high temperatures and low pressures.

As the gas is cooled, the curve no longer stays perfectly hyperbolic. At the critical temperature, Tc, the pV curve reaches a point with zero slope. Cooling farther creates a flat region where the volume can change without changing the pressure. This is the part of the curve where boiling and condensation occur.

In this transition region, a substance can expand as liquid changes into gas or contract as gas changes into liquid. The temperature and pressure stay the same during this change. To the left of the transition region, the curve is steep. This shows the liquid phase, which is almost incompressible, so a small decrease in volume needs a large increase in pressure.

The flat part of the curve represents liquid and gas coexisting. To the right of this region, the curve shows the gas phase. Isotherms above Tc do not pass through the liquid-gas transition. That is why liquid cannot exist above the critical temperature. At low enough pressure above Tc, the gas can have the density of a liquid but still not condense. This is called a supercritical gas. At higher pressure, the substance is solid. Carbon dioxide is one example, because it has no liquid phase above 31 degrees Celsius. The critical pressure is the highest pressure at which the liquid can exist, and the point at the critical pressure and critical temperature is the critical point.

Liquid-Gas Changes on pV Curves

equation of state

Gas Behavior in the Equation of State

The equation of state describes how a gas’s pressure, volume, temperature, and number of moles are related. These macroscopic properties help define the condition, or state, of the matter in a thermodynamics system. The relationship between these quantities can be written as a simple mathematical expression. In some cases, it is too complex to express in a formula. Even then, the link between the quantities still exists. When an equation of state cannot be written mathematically, scientists...

ideal gas equation

Gas Laws Behind the Ideal Equation

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van der waals equation

How Real Gases Deviate from Ideal Behavior

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pv-diagrams

pV curves show how gas pressure changes with volume. A pV diagram is a graph of pressure versus volume for the gas being studied. It helps describe how the substance behaves. When the gas acts like an ideal gas, the ideal gas equation gives the link between pressure and volume. A common pV curve is an isotherm, which is a line drawn at fixed temperature and fixed number of molecules. For an ideal gas, pressure times volume stays constant. That means volume goes down as pressure goes up. The...

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Avogadro's Number and Gas Particle Motion

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molecular kinetic energy

Gas Pressure and Molecular Motion

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distribution of molecular speeds

Molecular Speed Curves and Vapor Pressure

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maxwell-boltzmann distribution: problem solving

maxwell-boltzmann-distribution-problem-solving

Maxwell-Boltzmann Gas Speed Ratio

The Maxwell-Boltzmann distribution describes how molecular speeds are spread in a gas. Even though individual molecules move in random directions, the whole gas has a predictable speed pattern. This distribution is written as f(v), where v is molecular speed. The distribution function is used to find the expected number of particles with speeds between v1 and v2. Because N is dimensionless, f(v) has units of seconds per meter. The relationship can also be written in differential form for speed...

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Water Phase Changes on a Pressure Chart

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Gas collisions: path length and time

Gas collisions in a cylinder help explain the mean free path and mean free time. Gas molecules move in random motion. They collide with each other and change speed and direction. The mean free path is the average path length between collisions. The mean free path depends on how many molecules are packed into a volume. It varies inversely with density. When more molecules are present, collisions happen more often, so the mean free path becomes shorter. It also depends on molecule size. Larger...

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key terms and concepts

Explore how pV curves show ideal gas behavior, boiling, condensation, the critical point, and why carbon dioxide has no liquid phase above 31°C.

Liquid-Gas Changes on pV Curves | JoVE K12

physics

JoVE Core Física presenta la teoría y la aplicación de conceptos físicos fundamentales, como la cinemática, dinámica, mecánica de fluidos, estática, ondas y acústica, mediante animaciones audiovisuales concisas y fáciles de entender. Además, los vídeos de científicos en acción muestran la aplicación de los conceptos relacionados en experimentos de investigación clásicos y originales, realizados en laboratorios de todo el mundo.

Florida Department of Education

Physical Science

SC.912.P.12

SC.912.P.12.10

Georgia Standards of Excellence

9-12

SC5.

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Gas Laws: Pressure, Volume, Temperature, and Moles

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CHEM1.PS1.1

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CHEM1.PS1.2

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Perform stoichiometric calculations involving the following relationships: mole- mole; mass-mass; mole-mass; mole- particle; and mass- particle. Show a qualitative understanding of the phenomenon of percent yield, limiting, and excess reagents in a chemical reaction through pictorial and conceptual examples. (states of matter liquid and solid; excluding volume of gasses). EXPLANATION: This standard builds on the idea that balancing chemical reactions provides evidence for conservation of mass and that the behavior of atoms follows predictable patterns. Students now have the opportunity to utilize this understanding as they perform and evaluate chemical reactions. (The concepts of limiting reagent and percent yield are presented; however, students are not expected to determine these values algebraically. Use of molar volume in stoichiometric processes is beyond the scope of this standard.)

CHEM1.PS1.3

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Chemical Reactions in Aqueous Solutions

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Precipitation Reactions

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Oxidation-Reduction Reactions

Oxidation&ndash;Reduction Reactions

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Acids, Bases and Neutralization Reactions

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CHEM1.PS1.4

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Conduct investigations to explore and characterize the behavior of gasses (pressure, volume, and temperature), develop models to represent this behavior, and construct arguments to explain this behavior. Evaluate the relationship (qualitative and quantitatively) at STP between pressure and volume (Boyle's Law), temperature and volume (Charles' Law), temperature and pressure (Gay-Lussac Law) and moles and volume (Avogadro's Law), and evaluate and explain these relationships with respect to kinetic molecular theory. Be able to understand, establish, and predict the relationships between volume, temperature, and pressure using combined gas law both qualitatively and quantitatively. EXPLANATION: When exploring the behavior of gasses, it is important to consider experimental design. Experiments used to show the relationships between these sets of variables should include one independent and one dependent variable. Other variables should be held constant. Pressure should serve as the dependent variable because it cannot be manipulated directly. Avogadro's Law can be used to relate the amount of gas in two different containers in lieu of knowing actual number of gas particles in an individual container. Individual demonstrations can be performed to explore each of the different gas laws.

CHEM1.PS1.5

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CHEM1.PS1.7

Liquid-Gas Changes on pV Curves

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