Gases Boyle s law

The properties of gases. Boyle s law. The law of Charl i and Gay-Lussac. The absolute temperature scale. Avogadro s law. Standard (Yinditions. 

Ideal Gas Concept Measurement of Gases Boyle s Law Charles s Law Combined Gas Law A Clinical Perspective Autoclaves and the Gas Laws Avogadro s Law Molar Volume of a Gas Gas Densities The Ideal Gas Law An Environmental Perspective The Greenhouse Effect and Global Warming... 

The development of absolute temperatures began when quantitative experiments were made on the properties of gases. Boyle s law was long known. It states that for a given amount of gas the product of pressure and volume is constant for a given temperature, as summarized in Fig. 2.8. In 1802 Gay-Lussac found that gases expand linearly with temperature when measured with a mercury-in-glass thermometer. With these two observations it became possible to define a temperature that is independent... 

Pressure is an especially important variable with gases, because the volume of a quantity of gas at a fixed temperature is inversely proportional to pressure. The temperature/pressure/volume relationships of gases (Boyle s law, Charles law, and the general gas law) are discussed in Chapter 2. 

Robert Boyle (1627-1691), an Irish chemist, physicist, and inventor who discovered the inverse relationship of volume and pressure in gases (Boyle s law, V 1/p) and was the first to publish it in 1662. He made investigations into the expansive force of freezing water, on crystals, on electricity, and on hydrostatics, studied the chemistry of combustion, and conducted experiments in physiology. 

Ideal (or perfect) gas behavior is approached by most vapors and gases in the limit of low pressures and elevated temperatures. Two special forms of restricted utility known as the Boyle s law and the Charles law preceded the development of the perfect gas law. 

Pressure, temperature, and volume are properties of gases that are completely interrelated. Boyle s law and Charles law may be combined into one equation that is referred to as the ideal gas law. This equation is always true for ideal gases and is true for real gases under certain conditions. 

Kinetic theory A theory of matter based on the mathematical description of the relationship between pressures, volumes, and temperatures of gases (PVT phenomena). This relationship is summarized in the laws of Boyle s law, Charle s law, and Avogadro s law. 

Factors that would affect the slope of this straight line are related to deviations real gases exhibit from ideality. At higher pressures, real gases tend to interact more, exerting forces of attraction and repulsion that Boyle s Law does not take into account. 

Another great scientist who lived around the same time as Isaac, in the seventeenth century, was Robert Boyle. Robert discovered one of the fundamental laws about gases.This law, called Boyle s law, states that when pressure increases on a gas, the volume decreases (as long as the temperature stays the same). If you close the opening of a bicycle pump and press down on the handle, the volume decreases but the pressure increases. It gets harder and harder to push. Robert had discovered the law, but he didn t know why gases acted this way and no one else did either. 

Boyle, like many scholars of his day, studied and published in a number of areas including theology, philosophy, science, and political thought. In the area of chemistry, Boyle, in the tradition of van Helmont, studied gases. Aided by his assistant Robert Hooke, Boyle used a vacuum pump to conduct experiments in which he discovered air was necessary for life, sound does not travel in a vacuum, and that the volume of a gas is inversely proportional to pressure. This last discovery is one of the basic gas laws, and today is known as Boyle s Law (see Chapter 9). Boyle applied his work on gases to a study of the atmosphere and determined the density of air, and how atmospheric pressure changes with elevation. 

An attempt was made by Daniel Bernoulli (1738) to explain Boyle s law on tlie basis of what later became known as the kinetic theory of gases. Bernoulli introduced tlie concept that the pressure of a gas results from the collisions of gas molecules within tlie walls of the gas container. This established a connection between the numbers of gas molecules present and their kinetic energy present at any given temperature. 

BOYLE S LAW. This law, attributed to Robert Boyle (1662) but also known as Mariottc s law, expresses the isothermal pressure-volume relation for abody of ideal gas. That is, if the gas is kept at constant temperature, the pressure and volume are in inverse proportion, or have a constant product. The law is only approximately true, even for such gases as hydrogen and helium nevertheless it is very useful. Graphically, it is represented by an equilateral hyperbola (see Fig. I). If the temperature is not constant, the behavior of die ideal gas must be expressed by die Boyle-Charles law. 

Prediction 2, that such big molecules ought to be supercritical gases under ambient conditions, is supported by a more contentious argument based on their equation of state. The liquid state, and condensed phases in general, exist because of the short-range attractive forces between molecules. The simplest of all equations of state, Boyle s Law, PV = RT, makes no provision for attractive forces and does not predict condensed phases. The next approximation is Van der Waals equation ... 

Boyle s law can be derived from theoretical principles by making a few assumptions about the nature of gases. In the process, we obtain an important insight into the nature of temperature. 

Standard atmospheric pressure Pressure measurement Standard conditions Gas laws Boyle s law Charles law Gay-Lussac s law Combined gas law Density of an ideal gas Dalton s law of partial pressures Collecting gases over a liquid Deviations from ideal behavior... 

Rationalize Boyle s law in terms of the kinetic molecular theory of gases. 

From the earliest days of quantitative inquiry, scientists have sought to uncover the mathematical relationships that describe natural phenomena, including the properties of gases. Because there are four fundamental properties of a gas, namely, P, T, V, and n, discovering the relationship between any two requires that the other two properties be kept constant. Some of the earliest quantitative studies of gases were reported in the mid-1600s by British chemist Robert Boyle, who found that for a fixed amount of a gas at a specific temperature (i.e., constant n and T), the volume was inversely proportional to the applied pressure. This V-P relationship, known as Boyle s law, is represented as... 

Daniel Bernoulli proposed the kinetic molecular theory for gases in the early 1700s to explain the nature of heat and Boyle s Law. At that time, heat was thought to be related to the release of a substance called phlogiston from combustible material. 

The British scientist Robert Boyle made many contributions in the fields of medicine, astronomy, physics, and chemistry. However, he is best known for his work on the behavior of gases. In 1662, Boyle found that when the temperature is held constant, the pressure of a trapped amount of gas (any gas) is inversely proportional to its volume. That is, when the pressure of the gas increases, the volume of the gas decreases when the pressure of the gas decreases, the volume of the gas increases. Boyle s Law can be written mathematically as follows ... 

Robert Boyle was a seventeenth-century Irish scientist who studied the relationship between pressure and volume in gases. He confined his experimentation to these factors, without any change in temperature. As you visualize a situation in which only volume and pressure can change, think of a helium-filled balloon. If you squeeze the balloon to make it smaller, you can feel the pressure inside it become greater and greater. The balloon could even burst because of the pressure. In mathematical terms, Boyle s Law states that volume and pressure are inversely proportional. That is, as volume decreases, pressure increases. This law also means that as volume increases, pressure decreases. 

---