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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

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

Basit gaz yasaları, özellik çiftleri arasındaki ilişkileri açıklamak için diğerlerini sabit tutararak birbirine bağlı dört gaz özelliğini değiştirir. Boyle yasasına göre, bir gazın sıcaklığı ve mol sayısı sabit tutulduğunda, basınç ve hacim ters bir ilişki gösterir. Hacim azaldıkça gazın uyguladığı basınç artar.Bu nedenle P ve V'nin çarpımı bir sabite eşittir. İki farklı koşul altında, ilk basınç ve hacmin çarpımı ile son basınç ve hacmin çarpımı eşittir. Yani hacim ve mol sayısı sabit tutulursa, basınç ve sıcaklık doğrudan bir ilişki gösterir.Sıcaklık yükseldikçe, parçacıklar daha hızlı hareket eder ve daha sık yüksek enerjili çarpışmalara neden olurlar ve böylece basınç artar. P ve T oranı bu nedenle bir sabite eşittir. Bu, bazen Amontons yasası olarak adlandırılan Gay-Lussac yasasıdır.İki farklı koşul kümesi altında, ilk basınç ve sıcaklık oranı ile son basınç ve sıcaklık oranı eşittir. Ardından, sabit sayıda gaz molü ile şişirilmiş bir balon düşünün. Atmosferin dış basıncı sabittir.Charles yasasına göre, eğer moller ve basınç sabit tutulursa, gazın hacmi ve sıcaklığı Kelvin cinsinden doğrudan bir ilişki gösterir. Sıcaklığın artmasıyla, gaz parçacıkları daha hızlı hareket ederek daha fazla sayıda çarpışmaya neden olur ve balonun hacmini artırır. Aksine, sıcaklığın düşürülmesi balonun küçülmesine ve hacim olarak azalmasına neden olur.V ve T oranı bir sabite eşittir. İki farklı koşul altında, ilk hacim ve sıcaklığın oranı ve son hacim ve sıcaklığın oranı eşittir. Şimdi, balonun daha fazla hava ile şişirildiğini varsayalım.Avogadro yasasına göre, basınç ve sıcaklık sabit tutulduğunda, gazın hacmi ile mol sayısı doğrudan bir ilişki gösterir. Artan mol sayısı parçacıkları doldurur ve daha fazla sayıda çarpışmaya neden olur. Bu, balonu gaz parçacıklarını barındırmak için hacmini genişletmeye zorlar.Hacim ve mol sayısı oranı, bu nedenle, bir sabite eşittir. İki farklı koşul altında, başlangıç hacmi ve mol sayısı oranı ile son hacim ve mol sayısı oranı eşittir. Üç gaz yasasının ifadelerini birleştirmek ve orantılılık işaretini ideal gaz sabiti R ile değiştirmek, ideal gaz yasasını verir.R, tüm gazlar için aynı değere sahiptir ve mol Kelvin başına 8, 314 Joule veya mol-Kelvin başına 0, 08206 litre-atmosfere eşittir.

gaz yasaları

Bilim insanları deneyler ile ideal gaz için geçerli basınç ve sıcaklık, basınç ve hacim, hacim ve sıcaklık ve hacim ve mol gibi değişken çiftleri arasındaki matematiksel ilişkileri incelemiştir.
 
 <h4>Basınç ve Sıcaklık: Gay-Lussac yasası (Amontons Yasası)</h4>
 
 Bir basınç göstergesine bağlı sert bir kabı gazla doldurduğunuzu ve daha sonra gazın kaçmaması için kabı kapattığınızı düşünün. Eğer konteyner soğutulursa, içindeki gazın da aynı şekilde soğuduğu ve basıncının azaldığı görülmektedir. Kap sert ve sıkıca kapatıldığından, hem hacim hem de gaz mol sayısı sabit kalır. Küre ısıtılırsa, içindeki gaz ısınır ve basınç artar.
 
 Sıcaklık ve basınç doğrusal olarak ilişkilidir ve bu ilişki sabit bir hacimle sınırlı herhangi bir gaz örneği için gözlenir. Sıcaklık kelvin ölçeğinde ise, P ve T doğru orantılıdır (yine, hacim ve gaz molleri sabit tutulduğunda); kelvin ölçeğindeki sıcaklık belirli bir oranda artarsa, gaz basıncı da aynı oranda artar.
 
 Gazlar için bu basınç-sıcaklık ilişkisi Gay-Lussac yasası olarak bilinir. Bu yasa hacim sabit tutulduğunda gazın basıncının kelvin ölçeğinde sıcaklık ile doğru orantılı olduğunu söyler. Matematiksel olarak, bu şu şekilde yazılabilir:
 
 <img alt=""Eq1"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-01.png"" style=""height: 40px;"" />
 
 Burada k gazın türüne, miktarına ve hacmine bağlı olan bir oran sabitidir. Bu yüzden kapalı ve sabit hacimli bir gaz için P/T oranı sabittir (ör. P/T = k). Eğer gaz başlangıçta 'Durum 1'de ise (yani P = P1 ve T = T1) ve 'Durum 2'ye (yani P = P2 ve T = T2) geçerse
 
 <img alt=""Eq2"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-02.png"" style=""height: 40px;"" />
 
 Bu yüzden  
 
 <img alt=""Eq3"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-03.png"" style=""height: 40px;"" />
 
 Herhangi bir gaz kanunu hesaplaması için sıcaklıkların kelvin ölçeğinde olması gerektiğini unutmayın. 
 
 <h4>Hacim ve Sıcaklık: Charles Yasası</h4>
 
 Bir balon hava ile doldurulur ve kapatılırsa, balon atmosfer basıncında (1 atm) belirli bir miktarda hava içerir. Bu balon bir buzdolabına yerleştirilirse, içindeki gaz soğur ve balon küçülür (hem gaz miktarı hem de basıncı sabit kalır). Balon çok soğutulursa, büyük ölçüde küçülür. Isındığında, balon tekrar genişleyecektir.
 
 Bu durum sıcaklığın sabit basınçta belirli bir miktarda kapalı gazın hacmi üzerindeki etkisinin bir örneğidir. Sıcaklık arttıkça hacim artar ve sıcaklık azaldıkça hacim azalır.
 
 Sabit basınçta belirli bir gaz miktarının hacmi ve sıcaklığı arasındaki ilişki Charles yasası olarak bilinir. Bu yasa basıncı sabit tutulduğunda belirli bir miktar gazın hacmi ve kelvin ölçeğine göre sıcaklık arasında doğru orantı olduğunu söyler.
 
 Matematiksel olarak, bu şu şekilde yazılabilir:
 
 <img alt=""Eq4"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-04.png"" style=""height: 40px;"" />
 
 burada k gazın miktar ve basıncına bağlı olan oran sabitidir. Kapalı ve sabit basınç altındaki bir gazda V/T oranı sabittir.
 
 <h4>Hacim ve Basınç: Boyle Yasası</h4>
 
 Hava geçirmez bir şırınga kısmen hava ile doldurulursa, şırınga örneğin 25 °C gibi sabit bir sıcaklıkta belirli bir miktarda hava içerir. Sıcaklık sabit kalırken pistona yavaşça basılırsa, şırıngadaki gaz daha küçük bir hacme sıkıştırılır ve basıncı artar. Piston çıkarılırsa, gazın hacmi artar ve basınç azalır.
 
 Bir kabın hacminin azaltılması içerdiği gazın basıncını artıracak ve hacminin arttırılması basıncını azaltacaktır. Hacim belirli bir oranda artarsa, basınç aynı oranda azalır ve bunun tersi de geçerlidir. Bu nedenle, basınç ve hacim ters orantılılık gösterir: orantılılık: basıncın arttırılması, gazın hacminde bir azalmaya neden olur. Matematiksel olarak bu şu şekilde yazılabilir:
 
 <img alt=""Eq5"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-05.png"" style=""height: 40px;"" />
 
 burada k sabittir. P'ye karşılık V'nin grafiği bir hiperbole şeklindedir. Eğri çizgilere sahip grafiklerin, değişkenlerin düşük veya yüksek değerlerinde doğru bir şekilde okunması zordur ve teorik denklemlerin ve parametrelerin deneysel verilere uydurulmasında kullanılması daha zordur. Bu nedenlerden dolayı, bilim adamları genellikle verilerini "doğrusallaştırmanın" bir yolunu bulmaya çalışırlar. Grafiksel olarak, basınç ve hacim arasındaki ilişki, hacme karşı basıncın tersini veya basınca karşı hacmin tersini çizerek gösterilir.
 
 Sabit sıcaklıkta belirli bir gazın hacmi ve basıncı arasındaki ilişki Boyle yasası ile açıklanır: Sabit sıcaklıkta tutulan belirli bir gazın hacmi, ölçüldüğü basınçla ters orantılıdır.
 
 <h4>Gaz ve Mol Hacmi: Avogadro Yasası</h4>
 
 İtalyan bilim adamı Amedeo Avogadro, 1811'de gazların davranışını açıklamak için bir hipotez geliştirdi ve aynı sıcaklık ve basınç koşullarında ölçülen tüm gazların eşit hacimlerinin aynı sayıda molekül içerdiğini belirtti. Avogadro Yasası tarafından ifade edilen bu ilişki zamanla birçok deneysel gözlemle desteklenmiştir: Sınırlı bir gaz için, basınç ve sıcaklığın her ikisi de sabit kalırsa hacim (V) ve mol sayısı (n) doğru orantılıdır.
 
 Bu yasa denklem formunda, bu şu şekilde yazılır:
 
 <img alt=""Eq6"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-06.png"" style=""height: 40px;"" />
 
 Diğer değişken çiftleri için de matematiksel ilişkiler belirlenebilir, örneğin P ile n ve n ile T.
 
 <h4>İdeal Gaz Yasası</h4>
 
 Bu dört yasayı birleştirmek, ideal gaz yasasını, bir gazın basıncı, hacmi, sıcaklığı ve mol sayısı arasındaki ilişkiyi verir:
 
 <img alt=""Eq7"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-07.png"" style=""height: 40px;"" />
 
 Burada R, ideal gaz sabiti veya evrensel gaz sabiti olarak adlandırılan bir sabittir. Basınç, hacim ve sıcaklığı ifade etmek için kullanılan birimler, boyutsal analizin gerektirdiği şekilde gaz sabitinin uygun şeklini belirler. R'nin sıklıkla kullanılan halleri 0,08206 L⋅atm mol–1⋅K–1 ve 8,314 kPa⋅L mol–1⋅K–1'dir.
 
 P, V ve T özelliklerinin ideal gaz yasası (veya diğer gaz yasaları) tarafından doğru bir şekilde tanımlandığı gazların ideal davranış sergilediği veya ideal gazın özelliklerine yaklaştığı söylenir. İdeal bir gaz, sadece nispeten düşük basınç ve yüksek sıcaklık koşulları altında gazlar için makul olan varsayımsal bir yapıdır.
 
 İdeal gaz denklemi, gaz sabiti R ve değişken özellikler P, V, n ve T olmak üzere beş terim içerir. Bu terimlerden herhangi dördünün belirtilmesi, beşinci terimi hesaplamak için ideal gaz yasasının kullanılmasına izin verecektir.
 
 İdeal bir gazın mol sayısı iki farklı koşul kümesi altında sabit tutulursa, birleşik gaz yasası (atm, L ve K birimleri kullanılarak) olarak adlandırılan yararlı bir matematiksel ilişki elde edilir: 
 
 <img alt=""Eq8"" src=""https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-08.png"" style=""height: 40px;"" />
 
 Her iki durum da n × R çarpımına eşit olacaktır (burada n = gazın mol sayısı ve R ideal gaz yasası sabitidir).
 
 Bu metin bu kaynaktan uyurlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/9-2-relating-pressure-volume-amount-and-temperature-the-ideal-gas-law"">Openstax, Chemistry 2e, Section 9.2: Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law</a>.

Gaz Yasaları

Deneyler yoluyla, bilim adamları, basınç ve sıcaklık, basınç ve sıcaklık gibi değişken çiftleri arasındaki matematiksel ilişkileri kurdular ve ...

Education

JoVE Core

Kimya

Gases

Gazlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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

definition-measurement-pressure-atmospheric-pressure-barometer

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

applications-of-the-ideal-gas-law-molar-mass-density-and-volume

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

mixtures-of-gases-dalton-s-law-of-partial-pressures-and-mole-fractions

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

chemical-stoichiometry-gases-using-ideal-gas-law-to-determine

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

basic-postulates-kinetic-molecular-theory-particle-size-energy

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

kinetic-molecular-theory-gas-laws-explain-properties-gas

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

kinetic-molecular-theory-molecular-velocities-temperature-kinetic

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

behavior-gas-molecules-molecular-diffusion-mean-free-path

Gas Particle Motion, Diffusion, and Effusion

Gas particle motion, diffusion, and effusion explain how gases spread and escape in everyday settings. Gas molecules move at very high speeds, but they collide with other gas molecules and change direction many times before reaching a target. At room temperature, a gas molecule can experience billions of collisions each second. The mean free path is the average distance a molecule travels between collisions. This distance becomes larger when pressure decreases. In general, the mean free path...

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

real-gases-effects-intermolecular-forces-molecular-volume-deriving

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

chemistry

JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

ohios-learning-standards-and-model-curriculum

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

CHEM.10.B

Alabama Course of Study Science

9-12.C.1.4.e

9-12.C.4.7.b

Earth and Space Science

Earth's Systems

9-12.ESS.2.7.c

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-9.

Georgia Standards of Excellence

SC5.

gas-laws-pressure-volume-temperature-and-moles

Gas Laws: Pressure, Volume, Temperature, and Moles

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

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

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

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

Whether solid, liquid, or gas, a substance&#39;s state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the ...

phase-transitions-vaporization-and-condensation

Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

phase-transitions-sublimation-and-deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

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.

PS.Chm.7.1

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

Energy can be converted from one form into another, but all of the energy present before a change occurs always exists in some form ...

Internal Energy

The total of all possible kinds of energy present in a substance is called the internal energy (U), sometimes symbolized as E. Suppose a system with ...

Quantifying Heat

Thermal Energy&#160;

Microscopically, thermal energy is the kinetic energy associated with the random motion of atoms and molecules. Temperature is a ...

Quantifying Work

As a system undergoes a change, its internal energy can change, and energy can be transferred from the system to the surroundings, or from the ...

Enthalpy

Chemists ordinarily use a property known as enthalpy (H) to describe the thermodynamics of chemical and physical processes. Enthalpy is defined as the sum ...

Thermochemical Equations

For a chemical reaction (the system) carried out at constant pressure &ndash; with the only work done caused by expansion or contraction &ndash; the ...

Constant Pressure Calorimetry

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a ...

Constant Volume Calorimetry

Calorimeters are useful to determine the heat released or absorbed by a chemical reaction. Coffee cup calorimeters are designed to operate at constant ...

using-differential-scanning-calorimetry-to-measure-changes-in-enthalpy

Using Differential Scanning Calorimetry to Measure Changes in Enthalpy

Source: Laboratory of Dr. Terry Tritt &#8212; Clemson University
Differential Scanning Calorimetry (DSC) is a method of thermodynamic analysis based on ...

Hess's Law

There are two ways to determine the amount of heat involved in a chemical change: measure it experimentally, or calculate it from other experimentally ...

Standard Enthalpy of Formation

Enthalpy changes are typically tabulated for reactions in which both the reactants and products are at the same conditions. A standard state is a commonly ...

Enthalpies of Reaction

Hess&rsquo;s law can be used to determine the enthalpy change of any reaction if the corresponding enthalpies of formation of the reactants and products ...

Use mathematics and computational thinking to execute simple calorimetric calculations based on the Law of Conservation of Energy.

PS.Chm.7.2

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

Gas pressure is caused by force exerted by gas molecules colliding with the surfaces of objects. Although the force of each collision is very small, any ...

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and ...

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

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, &nbsp;suggests that the volume of a given quantity of gas ...

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

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other&rsquo;s pressure. Each gas ...

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

Description

Transcript

Tags

More videos by Standards