Name: how gas pressure, volume, and temperature change
Uploaded: 2020-09-03T13:38:26.000Z
Duration: 3 min 19 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.3

gas-laws-boyle-s-gay-lussac-charles-avogadro-s-and-ideal-gas-law

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Las leyes de los gases manejan las 4 propiedades interdependientes de los gases:presión, temperatura, volumen y número de moles, para obtener relaciones entre pares de propiedades mientras las otras se mantienen constantes. Según la ley de Boyle, cuando la temperatura y el número de moles de un gas se mantienen constantes, la presión y el volumen exhiben una relación inversa. Mientras el volumen disminuye, la presión que ejerce el gas aumenta.Por lo tanto, el producto de P por V es igual a una constante. Bajo dos tipos distintos de condiciones, el producto de la presión inicial por el volumen inicial, y el producto de la presión final por el volumen final son iguales. Ahora, si el volumen y el número de moles se mantienen constantes, la presión y la temperatura muestran una relación directa.A medida que la temperatura aumenta, las partículas se mueven a mayor velocidad y se producen colisiones de alta energía más frecuentemente, por lo que la presión aumenta. Por lo tanto, la proporción de P y T da como resultado una constante. Esta es la ley de Gay-Lussac, a la que a veces se le llama ley de Amontons.Bajo dos conjuntos distintos de condiciones, la proporción de la presión inicial y la temperatura inicial, y la proporción de la presión final y la temperatura final son iguales. Ahora, imaginemos un globo que se infla con un número fijo de moles de un gas. La presión externa de la atmósfera es constante.Según la ley de Charles, si los moles y la presión se mantienen constantes, el volumen y la temperatura de un gas en grados Kelvin exhiben una relación directa. Con un aumento de la temperatura, las partículas de gas se mueven más rápido, lo que da como resultado un número mayor de colisiones, y esto incrementa el volumen del globo. Por el contrario, disminuir la temperatura hace que el globo se contraiga y disminuya su volumen.La proporción de V y T es igual a una constante. Bajo dos conjuntos distintos de condiciones, la proporción del volumen inicial y la temperatura inicial, y la proporción del volumen final y la temperatura final son iguales. Ahora, supongamos que el globo se infla con más aire.De acuerdo con la ley de Avogadro, cuando la presión y la temperatura se mantienen constantes, el volumen del gas y el número de moles manifiestan una relación directa. El mayor número de moles empuja las partículas, lo que se traduce en un mayor número de colisiones. Esto obliga al globo a expandir su volumen para tener espacio donde contener a las partículas de gas.Por lo tanto, la proporción de volumen y número de moles es igual a una constante. Bajo dos conjuntos distintos de condiciones, la proporción de volumen inicial y número de moles inicial, y la proporción de volumen final y número de moles final son iguales. Combinar las expresiones de las tres leyes de los gases y remplazar el signo de proporcionalidad por la constante de los gases ideales, R, da como resultado la ley de los gases ideales.R tiene el mismo valor para todos los gases y es igual a 8, 314 julios sobre mol Kelvin o 0, 08206 litro-atm sobre mol-Kelvin.

las leyes de los gases

A través de experimentos, los científicos establecieron las relaciones matemáticas entre pares de variables, tales como presión y temperatura, presión y volumen, volumen y temperatura, y volumen y moles, que sirven para un gas ideal.
 
 <h4>Presión y temperatura: Ley de Gay-Lussac (Ley de Amontons)</h4>
 
 Imagine llenar un recipiente rígido fijado a un manómetro con gas y luego sellar el recipiente para que no escape el gas. Si el contenedor se enfría, el gas en el interior también se enfría y se observa que su presión disminuye. Dado que el contenedor es rígido y está sellado herméticamente, tanto el volumen como el número de moles de gas permanecen constantes. Si la esfera se calienta, el gas en el interior se calienta y la presión aumenta.
 
 La temperatura y la presión están relacionadas linealmente y esta relación se observa para cualquier muestra de gas confinada a un volumen constante. Si la temperatura está en la escala kelvin, entonces P y T son directamente proporcionales (de nuevo, cuando el volumen y los moles del gas se mantienen constantes); si la temperatura en la escala kelvin aumenta en un factor determinado, la presión del gas aumenta en el mismo factor.
 
 Esta relación presión-temperatura para los gases se conoce como ley de Gay-Lussac. La ley establece que la presión de una cantidad determinada de gas es directamente proporcional a su temperatura en la escala kelvin cuando el volumen se mantiene constante. Matemáticamente, esto se puede escribir como:
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-01.png" style="height: 40px;" />
 
 donde k es una constante de proporcionalidad que depende de la identidad, cantidad y volumen del gas. Para un volumen de gas limitado y constante, la relación P/T es por lo tanto constante (es decir, P/T= k). Si el gas se encuentra inicialmente en la “condición 1” (con P=P1 y T=T1) y cambia a la “condición 2” (con P=P2 y T=T2), entonces
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-02.png" style="height: 40px;" />
 
 Por lo tanto,  
 
 <img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-03.png" style="height: 40px;" />
 
 Tenga en cuenta que para cualquier cálculo de la ley de los gases, las temperaturas deben estar en la escala kelvin. 
 
 <h4>Volumen y Temperatura: Ley de Charles</h4>
 
 Si un globo se llena de aire y se sella, entonces el globo contiene una cantidad específica de aire a presión atmosférica (1 atm). Si el globo se coloca en un refrigerador, el gas en el interior se enfría y el globo se contrae (aunque tanto la cantidad de gas como su presión permanecen constantes). Si el globo se enfría mucho, se encogerá mucho. Cuando este se calienta, el globo se expande de nuevo.
 
 Este es un ejemplo del efecto de la temperatura sobre el volumen de una cantidad determinada de un gas confinado a presión constante. El volumen aumenta a medida que aumenta la temperatura y disminuye a medida que disminuye la temperatura.
 
 La relación entre el volumen y la temperatura de una determinada cantidad de gas a presión constante se conoce como ley de Charles. La ley establece que el volumen de una cantidad determinada de gas es directamente proporcional a su temperatura en la escala kelvin cuando la presión se mantiene constante.
 
 Matemáticamente, esto se puede escribir como:
 
 <img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-04.png" style="height: 40px;" />
 
 donde k es una constante de proporcionalidad que depende de la cantidad y presión del gas. Para un gas confinado a presión constante, la relación V/T es constante.
 
 <h4>Volumen y presión: La ley de Boyle</h4>
 
 Si una jeringa hermética está parcialmente llena de aire, entonces la jeringa contiene una cantidad específica de aire a una temperatura constante, digamos 25 °C. Si el émbolo es presionado lentamente mientras la temperatura permanece constante, el gas de la jeringa se comprime en un volumen más pequeño y su presión aumenta. Si se extrae el émbolo, el volumen del gas aumenta y la presión disminuye.
 
 Al disminuir el volumen de un gas contenido aumenta su presión y al aumentar su volumen disminuye su presión. Si el volumen aumenta en un determinado factor, la presión disminuye en el mismo factor y viceversa. Por lo tanto, la presión y el volumen presentan proporcionalidad inversa: Proporcionalidad: El aumento de la presión produce una disminución del volumen del gas. Matemáticamente esto puede ser escrito:
 
 <img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-05.png" style="height: 40px;" />
 
 donde k es una constante. Un gráfico deP versus V muestra una hipérbole. Los gráficos con líneas curvas son difíciles de leer con precisión a valores bajos o altos de las variables y son más difíciles de usar para ajustar ecuaciones teóricas y parámetros a datos experimentales. Por esas razones, los científicos a menudo tratan de encontrar una manera de “linealizar” sus datos. Gráficamente, la relación entre presión y volumen se muestra trazando la inversa de la presión frente al volumen, o la inversa del volumen frente a la presión.
 
 La relación entre el volumen y la presión de una determinada cantidad de gas a temperatura constante está dada por la ley de Boyle: El volumen de una determinada cantidad de gas que se mantiene a temperatura constante es inversamente proporcional a la presión bajo la cual se mide.
 
 <h4>Moles de Gas y Volumen: Ley de Avogadro</h4>
 
 El científico italiano Amedeo Avogadro presentó en 1811 una hipótesis para explicar el comportamiento de los gases, afirmando que los volúmenes iguales de todos los gases, medidos en las mismas condiciones de temperatura y presión, contienen el mismo número de moléculas. Con el tiempo, esta relación fue apoyada por muchas observaciones experimentales expresadas por la ley de Avogadro: Para un gas confinado, el volumen (V) y el número de moles (n) son directamente proporcionales si la presión y la temperatura permanecen constantes.
 
 En forma de ecuación, esto se escribe como:
 
 <img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-06.png" style="height: 40px;" />
 
 Las relaciones matemáticas también se pueden determinar para los otros pares de variables, como P versus n y n versus T.
 
 <h4>La ley de los gases ideales</h4>
 
 Al combinar estas cuatro leyes se obtiene la ley de los gases ideales, una relación entre la presión, el volumen, la temperatura y el número de moles de un gas:
 
 <img alt="Eq7" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-07.png" style="height: 40px;" />
 
 Aquí, R es una constante llamada la constante de gas ideal o la constante de gas universal. Las unidades utilizadas para expresar la presión, el volumen y la temperatura determinan la forma correcta de la constante de gas como requiere el análisis dimensional. Los valores más comunes de R son 0,08206 L⋅atm mol&minus1⋅K&minus1 y 8,314 kPa⋅L mol−1⋅K−1.
 
 Se dice que los gases cuyas propiedades de PV y T son descritas con precisión por la ley de los gases ideales (o las otras leyes de los gases) muestran un comportamiento ideal o aproximan los rasgos de un gas ideal. Un gas ideal es una construcción hipotética que sólo es razonable para gases en condiciones de presión relativamente baja y temperatura alta.
 
 La ecuación del gas ideal contiene cinco términos, la constante de gas R y las propiedades variables P,V, n y T. Especificar cuatro de estos términos permitirá el uso de la ley de los gases ideales para calcular el quinto término.
 
 Si el número de moles de un gas ideal se mantiene constante bajo dos conjuntos diferentes de condiciones, se obtiene una relación matemática útil llamada ley de los gases combinados (usando unidades de atm, L y K): 
 
 <img alt="Eq8" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-08.png" style="height: 40px;" />
 
 Ambos conjuntos de condiciones son iguales al producto de n × R (donde n = es el número de moles del gas y R es la constante de la ley de los gases ideales).
 
 Este texto ha sido adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/9-2-relating-pressure-volume-amount-and-temperature-the-ideal-gas-law">Openstax, Química 2e, Sección 9.2: Relacionando Presión, Volumen, Cantidad y Temperatura: La Ley de los Gases Ideales</a>.

Las Leyes de los Gases

A través de experimentos, los científicos establecieron las relaciones matemáticas entre pares de variables, como la presión y la temperatura, la presión y ...

Education

Educación

JoVE Core

Química

Gases

KEY TERMS AND CONCEPTS

TÉRMINOS Y CONCEPTOS CLAVE

how gas pressure, volume, and temperature change

Gas pressure, volume, temperature, and amount are linked by several gas laws. Scientists found these relationships by studying how a confined gas changes when one variable is held constant and another changes. These patterns apply to an ideal gas, which is a useful model for gases under low pressure and high temperature.

Gay-Lussac’s law, also called Amontons’s law, connects pressure and temperature. If gas is trapped in a rigid container, the volume and number of moles stay constant. When the gas is cooled, its pressure drops. When it is heated, its pressure rises. On the kelvin scale, pressure and temperature are directly proportional, so the ratio P/T stays constant.

Charles’s law describes the link between volume and temperature at constant pressure. A sealed balloon in a refrigerator shrinks because the gas inside gets colder. When the balloon warms, it expands again. In this case, the amount of gas and the pressure stay constant, while volume changes with temperature. On the kelvin scale, volume and temperature are directly proportional, so V/T remains constant.

Boyle’s law explains the relationship between pressure and volume at constant temperature. An airtight syringe shows this effect clearly. Pressing the plunger compresses the gas into a smaller volume and raises the pressure. Pulling the plunger out lets the gas expand and lowers the pressure. This is an inverse relationship, so a larger volume means a lower pressure. A graph of P versus V is a hyperbola, which is hard to read at very high or low values. Scientists often linearize the data by plotting inverse pressure or inverse volume instead.

Avogadro’s law connects volume and the number of moles of gas. Amedeo Avogadro proposed in 1811 that equal volumes of gases, measured at the same temperature and pressure, contain the same number of molecules. For a confined gas, volume and moles are directly proportional when pressure and temperature stay constant. Other pairs of variables, such as pressure versus moles and moles versus temperature, can also be related.

The ideal gas law combines these relationships into one equation that links pressure, volume, temperature, and moles. It uses the gas constant R, which has different values depending on the units, such as 0.08206 L·atm mol−1·K−1 or 8.314 kPa·L mol−1·K−1. Gases that closely follow this model show ideal behavior. The ideal gas law uses five terms, so knowing any four lets you solve for the fifth. If the number of moles stays the same, the combined gas law is also useful for comparing two sets of gas conditions.

How Gas Pressure, Volume, and Temperature Change

how-gas-pressure-volume-and-temperature-change

definition and measurement of pressure: atmospheric pressure, barometer, and manometer

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Pressure Units and Tools for Gas Measurement

Pressure is the force applied to a given area, and gas pressure comes from gas molecules colliding with surfaces. Each collision is tiny, but many collisions over a small area can create high pressure. Pressure increases when force increases or when the area gets smaller. It decreases when force drops or when the area gets larger. Pressure is measured in pascals, or Pa, in the SI system. One pascal equals 1 newton per square meter, and a newton is a unit of force equal to 1 kg·m/s2. A pascal...

gas laws: boyle's, gay-lussac, charles', avogadro's, and ideal gas law

Gas pressure, volume, temperature, and amount are linked by several gas laws. Scientists found these relationships by studying how a confined gas changes when one variable is held constant and another changes. These patterns apply to an ideal gas, which is a useful model for gases under low pressure and high temperature. Gay-Lussac’s law, also called Amontons’s law, connects pressure and temperature. If gas is trapped in a rigid container, the volume and number of moles stay constant. When the...

applications of the ideal gas law: molar mass, density, and volume

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Ideal Gas Law at STP and Gas Density

The ideal gas law links pressure, volume, number of moles, and temperature. It helps explain how gas volume changes when pressure or temperature changes. At standard temperature and pressure, or STP, the values are 273.15 K and 1 atm. At STP, one mole of an ideal gas occupies about 22.4 L. This is called the standard molar volume. The gas can be hydrogen, oxygen, argon, or carbon dioxide, and the volume is still about 22.4 liters. Half a mole occupies 11.2 L, and 2 moles occupy 44.8 L. The...

mixtures of gases: dalton's law of partial pressures and mole fractions

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Gas Pressure in Mixtures: Partial Pressures

Gas pressure in mixtures is described by partial pressure and mole fraction. When gases do not chemically react, each gas in the mixture acts as if it were alone in the container. The pressure from one gas is called its partial pressure. For a mixture of three gases, A, B, and C, the total pressure equals the sum of their partial pressures: PA, PB, and PC. This is Dalton's law of partial pressures. It states that the total pressure of a mixture of ideal gases is the sum of the pressures from...

chemical stoichiometry and gases: using ideal gas law to determine moles

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Stoichiometry of Gases with the Ideal Gas Law

Chemical stoichiometry links the amounts of reactants and products in a chemical reaction. For gases, those amounts can also be measured by volume. If a gas’s volume, pressure, and temperature are known, the ideal gas equation can be used to find the number of moles present. The same idea works in reverse. If the moles of a gas are known, its volume can be found at any temperature and pressure. The transcript gives an example using 8.88 g of gallium reacting with excess hydrochloric acid.

basic postulates of kinetic molecular theory: particle size, energy, and collision

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Kinetic Molecular Theory and Gas Behavior

Kinetic molecular theory explains gas behavior at the particle level. It gives a microscopic model for what happens when pressure or temperature changes. Gas laws describe how macroscopic properties change, but they do not explain why those changes happen. The theory was put into a complete form by Rudolf Clausius in 1857. It was built from hundreds of experimental observations about gases. Those observations helped explain the different gas laws through a few basic postulates. One key idea...

kinetic molecular theory and gas laws explain properties of gas molecules

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Gas Pressure Patterns in Kinetic Molecular Theory

Kinetic molecular theory explains gas pressure by linking it to the motion of gas molecules. Gas pressure comes from rapidly moving molecules hitting the walls of a container. It depends on how many molecules strike a unit area in a given time. The theory also helps explain the main gas laws. In Gay-Lussac’s law, also called Amontons’s law, raising temperature increases the average speed and kinetic energy of gas molecules. If volume stays constant, the molecules collide with the walls more...

kinetic molecular theory: molecular velocities, temperature, and kinetic energy

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Gas Particle Speed Distributions and Temperature

Gas particle speed distributions and temperature are key ideas in the kinetic molecular theory. This theory explains the gas laws by describing how gas molecules move, collide, and share energy. Gas molecules do not all move at the same speed. A gas sample has an average speed and an average kinetic energy, but individual molecules move at different speeds. Their collisions are elastic, which means momentum is conserved. Because so many molecules collide, the overall speed distribution stays...

behavior of gas molecules: molecular diffusion, mean free path, and effusion

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Gas Particle Motion, Diffusion, and Effusion

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real gases: effects of intermolecular forces and molecular volume deriving van der waals equation

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Real Gases: When the Ideal Gas Law Breaks Down

Real gases are gases that do not always follow the ideal gas law, PV = nRT, especially when pressure is high or temperature is low. The ideal gas model assumes gas particles have no attractive or repulsive forces and take up negligible space compared with the container. At room temperature and 1 atm or less, many gases behave close to ideally. When conditions change, the measured relationships between pressure, volume, and temperature can drift away from the ideal prediction. One way to see...

key terms and concepts

Explore Boyle’s, Charles’s, Gay-Lussac’s, and Avogadro’s laws with simple gas examples, plus the ideal gas law for pressure, volume, temperature, and moles.

How Gas Pressure, Volume, and Temperature Change | JoVE K12

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JoVE Core Química da vida a los conceptos de química general mediante lecciones de vídeo basadas en animaciones, concisas y fáciles de entender. Además, en los vídeos de científicos en acción, se muestran experimentos de investigación clásicos y originales realizados en laboratorios de todo el mundo.

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Gas laws

Tennessee Academic Standards

High School

Matter and Its Interactions

CHEM1.PS1.5

CHEM1.PS1.6

Virginia  Standards of Learning

HIgh School

CH.6

CH.6.b

Minnesota Academic Standards in Science

2.2.1 9C.1.2.1.1

Arizona Science Standards

Physical Science

HS+C.P1

HS+C.P1U1.3

Texas Essential Knowledge and Skills

CHEM.10

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Alabama Course of Study Science

9-12.C.1.4.e

9-12.C.4.7.b

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Earth's Systems

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New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-9.

Georgia Standards of Excellence

SC5.

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Gas Laws: Pressure, Volume, Temperature, and Moles

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Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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Physical and Chemical Properties of Matter

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Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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surface-tension-capillary-action-and-viscosity

Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

States of Matter and Phase Changes

The internal energy of a substance&#8212;the total kinetic energy of all its molecules and the potential energy of their associated forces&#8212;depends ...

Phase Transitions

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Phase Transitions: Vaporization and Condensation

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Vapor Pressure

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Clausius-Clapeyron Equation

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Phase Transitions: Melting and Freezing

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Phase Transitions: Sublimation and Deposition

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Heating and Cooling Curves

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Phase Diagrams

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Use models to explain how changes in energy affect the arrangement and movement of the particles in solids, liquids, and gases, as well as the relative strengths of their intermolecular forces.

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Energy Basics

Chemical reactions, such as those that occur when you light a match, involve changes in energy as well as matter.

Chemical changes and their accompanying ...

First Law of Thermodynamics

Energy Conservation

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Internal Energy

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Quantifying Heat

Thermal Energy&#160;

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Quantifying Work

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Enthalpy

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Thermochemical Equations

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Constant Pressure Calorimetry

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Constant Volume Calorimetry

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Using Differential Scanning Calorimetry to Measure Changes in Enthalpy

Source: Laboratory of Dr. Terry Tritt &#8212; Clemson University
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Enthalpies of Reaction

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PS.Chm.7.2

Definition and Measurement of Pressure: Atmospheric Pressure, Barometer, and Manometer

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Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

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Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

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Chemical Stoichiometry and Gases: Using Ideal Gas Law to Determine Moles

Chemical stoichiometry describes the quantitative relationships between reactants and products in chemical reactions.

In addition to measuring quantities ...

Basic Postulates of Kinetic Molecular Theory: Particle Size, Energy, and Collision

The ideal-gas equation, which is empirical, describes the behavior of gases by establishing relationships between their macroscopic properties. For ...

Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws ...

Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

The kinetic molecular theory qualitatively explains the behaviors described by the various gas laws. The postulates of this theory may be applied in a ...

Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many ...

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and ...

Ideal Gas Law

Source: Laboratory of Dr. Andreas Z&#252;ttel - Swiss Federal Laboratories for Materials Science and Technology
The ideal gas law describes the behavior ...

Derivation of the Ideal Gas Law
Gases are a fundamental state of matter. A gas is a collection of molecules that have a significant distance between their ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
	According to the ideal gas law for a given ...

Use mathematics and computational thinking to explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitatively and quantitatively.

Understand the relationship among pressure, temperature, volume, and phase.

How Gas Pressure, Volume, and Temperature Change

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