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

単純気体の法則は 圧力 温度 体積 モル数の 4つの相互依存性のある 気体の性質を操作して 他の性質を一定に保ちながら 性質のペア間の関係を 導き出します ボイルの法則によれば 気体の温度とモル数が 一定であれば 圧力と体積は 逆の関係を示します 体積が減少すると ガスの圧力は増加します したがって PとVの積は 定数になります 2つの異なる条件では 初期圧力と体積の積と 最終圧力と体積の積は 等しくなります 体積とモル数が 一定であれば 圧力と温度は 直接関係があります 温度が上昇すると 粒子の移動速度が速くなり 高エネルギーの衝突が 頻繁に起こり 圧力が上昇します そのため PとTの比は 一定になります これがゲイ・リュサックの法則で アモントンの法則と 呼ばれることもあります 2つの異なる 条件セットの下では 初期圧力と温度の比と 最終圧力と温度の比は 等しくなります 次に 一定のモル数の 気体で膨らませた 風船を考えてみましょう 大気の外圧は一定である とします シャルルの法則によれば モル数と圧力が一定であれば 気体の体積と温度は ケルビン単位で直接関係を 示します 温度が上がると 気体の粒子の動きが速くなり 衝突の回数が増えて 風船の体積が増えます 一方 温度が下がると 風船は収縮して 体積が減少します V と T の比は 定数に等しくなります 2つの異なる条件では 初期体積と温度の比と 最終体積と温度の比は 等しくなります さて 風船をより多くの 空気で膨らませたとします アボガドロの法則によれば 圧力と温度が一定であれば 気体の体積とモル数は 直接関係があります モル数が増えると 粒子が混ざり合い 衝突の回数が増えます これにより 風船は ガス粒子を収容するために 体積を 膨張させざるを得なくなります したがって 体積とモル数の比は 一定になります 2つの異なる条件では 初期体積とモル数の比と 最終体積とモル数の比は 等しくなります 3つの気体の法則の式を 組み合わせ 理想気体定数Rを 組み込んで 比例符号を置き換えると 理想気体の状態 方程式が得られます Rはすべての気体で 同じ値を持ち 1モルケルビンあたり 0.08206リットルアトム または 1モルケルビンあたり 8.314ジュールです

気体の状態方程式

科学者たち実験によって、圧力と温度、圧力と体積、体積と温度、体積とモル数などの変数のペアの間に、理想気体をを成立させる数学的関係を確立しました。 
 
 <h4>圧力と温度：ゲイ・リュサックの法則（アモントンの法則） </h4>
 
 圧力計を取り付けた硬質容器に気体を充填し、気体が漏れないように容器を密閉します。 容器が冷却されると、内部のガスも同様に冷たくなり、圧力が低下することが観察されます。 容器は頑丈で密閉されているため、気体の体積とモル数は一定です。 容器が加熱されると、内部の気体は高温になり、圧力が上昇します。 
 
 温度と圧力は直線的な関係にあり、この関係は一定の体積に制限された気体の試料で観察されます。 温度がケルビンスケールであれば、P と T は正比例する（気体の体積とモル数が一定に保たれている場合）。ケルビンスケールの温度がある係数で上昇すると、気体の圧力も同じ係数で上昇します。 
 
 この気体の圧力温度関係は、ゲイ・リュサックの法則と呼ばれています。 この法則では、体積が一定に保たれている場合、所定の量の気体の圧力はケルビンスケールの温度に正比例すると規定されています。 数学的には、次のように記述できます。 
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-01.png" style="height: 40px;" />
 
 ここで、 k は気体の 種類 、量、体積に依存する比例定数です。 閉じ込められた一定の気体の体積の場合、比率 P/T は一定となります（つまり、 P/T = k ）。 気体が最初に「条件 1 」（P = P1 と T = T1）になっていて、「条件 2 」（P = P2 と T = T2）に変化した場合は、次のようになります 
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-02.png" style="height: 40px;" />
 
 したがって、  
 
 <img alt="Eq3" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-03.png" style="height: 40px;" />
 
 気体法則の計算では、温度はケルビンスケールでなければならないことに注意してください。  
 
 <h4>体積および温度 : チャールズの法則 </h4>
 
 バルーンが空気で満たされ、密閉されている場合、バルーンには大気圧（ 1 atm ）で一定の量の空気が含まれます。 バルーンを冷蔵庫に入れると、内部の気体が冷たくなり、バルーンが収縮します（気体の量と圧力は一定）。 気球が非常に冷たくなれば、かなり縮まります。 一方温められると、バルーンは再び拡張します。 
 
 これは、一定の圧力で一定量の密閉気体の体積に対する温度の影響の例です。 温度が上昇すると体積が増え、温度が低下すると体積は減ります。 
 
 一定圧力での特定の量の気体の体積と温度の関係は、チャールズの法則と呼ばれます。 この法則では、圧力が一定に保たれている場合、所定の気体の量はケルビンスケールの温度に正比例すると規定されています。 
 
 数学的には、次のように記述できます。 
 
 <img alt="Eq4" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-04.png" style="height: 40px;" />
 
 ここで、 k は気体の量と圧力に依存する比例定数です。 一定圧力の閉塞気体の場合、比率V/T は一定です。 
 
 <h4>体積と圧力：ボイルの法則 </h4>
 
 気密性の高いシリンジに空気が部分的に充填されている場合、シリンジには一定の温度（ 25 ° C など）で一定量の空気が入っています。温度が一定に保たれている間にプランジャーをゆっくりと押すと、シリンジ内の気体はより小さな量に圧縮され、圧力が上昇します。 プランジャを引くと、ガスの量が増加し、圧力が低下します。 
 
 含まれている気体の量を減らすと圧力が上昇し、量を増やすと圧力が低下します。 体積が特定の係数だけ増加すると、圧力は同じ係数で減少します。また、その逆も同様です。 そのため、圧力と体積は反比例の関係にあります。圧力を上げると、ガスの体積が減少します。 数学的には、次のように記述できます。 
 
 <img alt="Eq5" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-05.png" style="height: 40px;" />
 
 ここで、k は定数です。 P 対V のプロットは双曲線を描きます。 曲線を持つグラフは、変数の低値または高値で正確に読み取ることが困難であり、理論的な方程式やパラメータを実験データに適合させるのに使いにくくなっています。 このような理由から、科学者はデータを「線形化」する方法を見つけようとすることがよくあります。 圧力と体積の関係は、体積に対する圧力の反比例、または体積対圧力の逆数をプロットすることで、図示されます。 
 
 温度が一定の場合の気体の体積と圧力の関係は、ボイルの法則によって示されます。一定の温度における一定の気体の体積は、測定される圧力に反比例します。 
 
 <h4>気体のモル数と体積 : アボガドロの法則 </h4>
 
 イタリアの科学者、アメデオ・アボガドロは、 1811 年に気体の挙動を考慮して仮説を立て、温度と圧力の同じ条件で測定されたすべての気体の体積が同じ分子数を含むことを示しました。 時間の経過とともに、この関係はアボガドロの法則で示されている多くの実験的観測によって支持されました。閉じ込められた気体の場合、圧力と温度が一定であれば体積（ V ）とモル数（ n ）は正比例します。 
 
 方程式形式では、次のように記述されます。 
 
 <img alt="Eq6" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-06.png" style="height: 40px;" />
 
 P 対 n 、n 対Tなど、他の変数ペアの数学的関係も決定できます。
 
 <h4>理想気体の状態方程式 </h4>
 
 これらの 4 つの法則を組み合わせることで、気体の圧力、体積、温度、およびモル数の関係を示す理想気体の状態方程式が得られます。 
 
 <img alt="Eq7" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-07.png" style="height: 40px;" />
 
 ここでR は理想気体定数または普遍的気体定数と呼ばれる定数です。 圧力、体積、および温度を表すために使用される単位によって、次元解析で必要とされる気体定数の適切な形式が決まります。 R の最も一般的な値は、 0.08206 L × atm mol – 1 × K – 1 および 8.314 kPa × L mol – 1 × K – 1 です。 
 
 P 、 V 、およびTの特性が理想気体の状態方程式（またはその他の気体法則）によって正確に記述されている気体は、理想的な動作を示すか、理想気体の特性に近似すると言われています。 理想気体とは、比較的低圧で高温の条件下での気体にのみ適応できる仮説上の構成概念です。 
 
 理想気体の状態方程式には、 5 つの項目、気体定数 R 、および変数 P 、 V 、 n 、 T が含まれます。これらの項のいずれか 4 つを指定すると、理想気体の状態方程式を使用して 5 番目の項目を計算できます。 
 
 理想気体のモル数が 2 つの異なる条件で一定に保たれている場合は、（ atm 、 L 、 K の単位を使用して）複合気体法則（ボイル=シャルルの法則）と呼ばれる便利な数学的関係が得られます。  
 
 <img alt="Eq8" src="https://www.jovecore.com/CDNSource/lessons/1036/1036_Equations-08.png" style="height: 40px;" />
 
 両方の条件は n × R の積に等しくなります（ n は気体のモル数、 R は理想気体法則の定数）。 
 
 本書は <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 ：圧力、体積、量、および温度の関連：理想気体の法則から引用</a>したものです。

実験を通じて、科学者たちは、圧力と温度、圧力など、変数のペア間の数学的関係を確立しました...

Education

JoVE Core

化学

Gases

気体

KEY TERMS AND CONCEPTS

主要用語と概念

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

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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

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

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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

chemistry

JoVE Core 化学は、簡潔で理解しやすいアニメーションビデオレッスンを使用して、一般的な化学の概念を生き生きとしたものにします。さらに、活動する科学者のビデオでは、現在世界中の実験室で行われている古典的そして独創的な研究・実験をお見せします。

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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

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.

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Gas Laws: Pressure, Volume, Temperature, and Moles

Classifying Matter by State

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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 ...

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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 ...

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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

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Intermolecular Forces

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

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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, ...

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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 ...

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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

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