Boyle’s Law At constant temperature, the

Boyle s law At constant temperature the volume of a given mass of gas is inversely proportional to the pressure. Although exact at low pressures, the law is not accurately obeyed at high pressures because of the finite size of molecules and the existence of intermolecular forces. See van der Waals equation. 

Boyle s Law (at constant temperature) The volume of a gas (maintained at constant temperature) decreases as its pressure increases (P alA ) ... 

Boyle s law at constant temperature the volume V occupied by a given number of moles of gas varies in inverse proportion to the pressure p. That is to say... 

Boyle s Law At constant temperature, the volume occupied by a given mass of a gas is inversely proportional to the applied pressure. 

Conclusion and statement of the law. The generalization of Boyle s observations is known as Boyle s law at constant temperature, the volume occupied by a fixed amount of gas is inversely proportional to the applied (external) pressure, or... 

Boyle s law At constant temperature, the volume of a fixed number of moles of gas is... 

Boyle s Law. At constant temperature (T), the volume (V) of a fixed mass of an ideal gas is inversely proportional to the absolute pressure (P). That is,... 

For an ideal gas flowing through a column or channel we have modified Boyle s law, pV= constant, to the form p(v) = constant. Prove that this modification is valid at constant temperature under steady flow conditions using the general flux expression (Eq. 3.14) in the form... 

Ideal or perfect gases obey Boyle s law at all temperatures. This fact was established by Boyle and Mariotte in 1662. According to this law, the product of P and V is constant for a given mass of gas at a constant temperature, where P is the pressure of the gas and V is its volume. 

Alveolar pressure (Palv) is the pressure within the alveoli. In between breaths, it is equal to 0 cmH20. Because no pressure gradient exists between the atmosphere and the alveoli, there is no airflow. However, in order for air to flow into the lungs, alveolar pressure must fall below atmospheric pressure. In other words, alveolar pressure becomes slightly negative. According to Boyle s law, at a constant temperature, the volume of a gas and its pressure are inversely related ... 

A) Remember Boyle s law As the volume decreases (at constant temperature), the pressure increases. 

Boyle (1662) observed that at constant temperature the volume of a sample of gas varies inversely with pressme, but Boyle did not explain why this was so. Somewhat later. Charles (1787) refined the observation to the effect that the volume of any sample of a gas vanes directly with the absolute temperature provided thal the pressure is held constant. A few years later, Gay-Lussac (1808), in reporting the results of his experiments with reacting gases, observed that volumes of gases that are used or produced in a chemical reaction can be expressed in ratios of small whole numbers—a concept to become known as Gay-Lussac s law of combining volumes. It should be noted that tlie foregoing concepts proposed by Boyle, Charles, and Gay-Lussac were based upon experimental observations, not on theory. 

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. 

One common use of Boyle s law is to predict the new volume of a gas when the pressure is changed (at constant temperature), or vice versa. 

This gauge is used to measure low pressures within the range 10 tort to 1 x 10 torr. It is assumed that dry gases at low pressures obey Boyle s law, which states that the pressure of a given mass of gas, kept at constant temperature, is inversely proportional to its volume. 

To find the law of expansion under variable pressure, we must combine the above equations with Boyle s law. Boyle s law states that when we compress or dilate a gas at constant temperature, the volume and the pressure are inversely proportional to one another. The product pv, therefore, does not vary, i.e.. ... 

Figure 9 shows what happens to the gas molecules in a car cylinder as it compresses. As the volume decreases, the concentration, and therefore pressure, increases. This concept is shown in graphical form in Figure 10. The inverse relationship between pressure and volume is known as Boyle s law. The third column of Table 2 shows that at constant temperature, the product of the pressure and volume of a gas is constant.

Can this reaction be forced to produce more methane by changing the volume of the reaction vessel Suppose the vessel s volume can be changed using a piston-like device similar to the one shown in Figure 18-8. If the piston is forced downward, the volume of the system decreases. You have learned that Boyle s law says that decreasing the volume at constant temperature increases the pressure. The increased pressure is a stress on the reaction at equilibrium. How does the equilibrium respond to the disturbance and relieve the stress ... 

When the volume of a gas is plotted against its pressure at constant temperature, the resulting curve is one branch of a hyperbola. Figure 12-4b is a graphic illustration of this inverse relationship. When volume is plotted versus the reciprocal of the pressure, /P, a straight line results (Figure 12-4c). In 1662, Boyle summarized the results of his experiments on various samples of gases in an alternative statement of Boyle s Law ... 

Figure 12-10 A molecular interpretation of Boyle s Law— the change in pressure of a gas with changes in volume (at constant temperature). The entire apparatus is enclosed in a vacuum. 

Robert Boyle (1627-1691) studied the effect of changing the pressure of a gas on its volume at constant temperature. He concluded that at constant temperature, the volume of a given sample of gas is inversely proportional to its pressure. This is known as Boyle s law. It means that as the pressure increases, the volume becomes smaller by the same factor. That is, if the pressure is doubled, the volume is halved. This relationship can be expressed mathematically by any of the following ... 

Boyle s law, PV = constant, which states that for a given mass at fixed temperature the pressure (P) times the volume (V) of a gas is a constant ... 

Boyle s law (V l/P). Gas molecules are points of mass with empty space between them (postulate 1), so as the pressure exerted on the sample increases at constant temperature, the distance between molecules decreases, and the sample volume decreases. The pressure exerted by the gas increases simultaneously because in a smaller volume of gas, there are shorter distances between gas molecules and the walls and between the walls themselves thus, collisions are more frequent (Figure 5.13). The fact that liquids and solids cannot be compressed means there is little, if any, free space between the molecules. 

One common use of Boyle s law is to predict the new volume of a gas when the pressure is changed (at constant temperature), or vice versa. Because deviations from Boyle s law are so slight at pressures close to 1 atm, in our calculations we will assume that gases obey Boyle s law (unless stated otherwise). 

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