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Boyles’law

Boyle s law states that the volume of a fixed amount of gas at a constant temperature is inversely proportional to the pressure, provided the temperature does not change. It has been observed that, at a constant temperature, doubling the pressure on a sample of gas reduces the volume by one-half. Conversely, halving the pressure on a sample of gas results in a doubling of the volume. [Pg.109]

The graphical plot of pressure versus volume shows an inverse variation. In an inverse relationship, as the magnitude of one quantity increases, the magnitude of the second quantity decreases. This relationship may be expressed as [Pg.109]

The procedure in this lab is done using an air sample over water, and water vapor will saturate and add to the pressure. So, the water vapor pressure must be subtracted from the barometric pressure. You will consult the CRC Handbook of Chemistry and Physics to determine water vapor pressure at the temperature of the water being used in the activity. [Pg.109]

Additionally, the pressure equivalent of the heights of the water above and below the initial point must be calculated and either added to or subtracted from the corrected pressure for each case. Because mercury is 13.6 times as dense as water, any column of water can be converted to mm Hg, or torr, by dividing the water column height, in mm, by 13.6. Water is used instead of mercury because liquid mercury and its vapors are highly toxic and cannot be safely used in the classroom laboratory. [Pg.109]

For a sample of gas at a constant temperature, how does the product of pressure times volume compare at different pressures  [Pg.109]

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 [Pg.144]

The constant is the same for the great majority of gases. Thus, tripling the external pressure reduces the volume to one-third its initial value halving the external pressure doubles the volume and so forth. [Pg.144]

The wording of Boyle s law focuses on external pressure. In his experiment, however, adding more mercury caused the mercury level to rise until the pressure of the trapped air stopped the rise at some new level. At that point, the pressure exerted on the gas equaled the pressure exerted by the gas. In other words, by measuring the applied pressure, Boyle was also measuring the gas pressure. Thus, when gas volume doubles, gas pressure is halved. In general, if V gas increases, Pgas decreases, and vice versa. [Pg.144]

One question raised by Boyle s work was why the pressure-volume relationship holds only at constant temperature. It was not until the early 19 century, through the separate work of the French scientists J. A. C. Charles and J. L. Gay-Lussac, that the relationship between gas volume and temperature was clearly understood. [Pg.144]

During the seventeenth, eighteenth, and nineteenth centuries, scientists performed a number of experiments to determine the relationships among the variables listed in Table 21.1. The laws of gases are usually referred to by the names of their discoverers and are called Boyle s law, Charles s law, Avogadro s law, Dalton s law, Graham s law, and the ideal gas law. [Pg.228]

Robert Boyle (1627-91) was an Irish natural philosopher who studied the quantitative relationship between the pressure and volume of a gas. What he discovered was that the product of pressure times volume (P x V) is a constant if the quantity of gas (n) and the temperature (T) are both held constant. [Pg.228]

Oftentimes, Boyle s law is also stated as Pj Vj = P V. This says that when the quantity of gas and the temperature of the gas remain fixed, the volume of a gas is inversely proportional to the pressure applied to the gas. Increase the pressure (squeeze hard on a balloon) and the volume decreases (the balloon becomes smaller) decrease the pressure and the volume increases. [Pg.228]

Boyle s law states that pressure times volume is a constant for a fixed quantity of gas. In other words, as pressure increases, volume decreases as pressure decreases, volume increases. This is only true, however, if the temperature of the gas stays constant. Boyle s law only applies to gases in balloons or in other containers in which volume can change, not in containers with rigid walls like a metal box. [Pg.228]

Jacques Alexandre Cesar Charles (1746-1823) was a French scientist who was interested in both the behavior of gases and the behavior of balloons, the latter of which were just being developed when Charles was in his early thirties. [Pg.228]

Through a series of experiments, Robert Boyle (1627-1691) determined the relationship between the pressure (P) and volume (V) of a particular quantity of a gas. This relationship of P and V is known as Boyle s law Boyle s law [Pg.257]

At constant temperature (T), the volume (V) of a fixed mass of a gas is inversely proportional to the pressure (P), which may he expressed as [Pg.257]

Graph of pressure versus volume showing the inverse PV relationship of an ideal gas. [Pg.257]

When Boyle doubled the pressure on a specific quantity of a gas, keeping the temperature constant, the volume was reduced to one-half the original volume when he tripled the pressure on the system, the new volume was one-third the original volume and so on. His work showed that the product of volume and pressure is constant if the temperature is not changed  [Pg.257]

Note that the product of the pressure times the volume is the same number in each case, substantiating Boyle s law. We may then say that [Pg.257]

The second edition of Boyle s first book, New Experiments Physico-Mechanical Touching the Air, was published in 1662 and contained a section titled A Defense of Mr. Boyle s Explications of his Physico-mechanical Experiments, against Franciscus Linus. In this section, he disclosed the relationship between the pressure and the volume of a gas that we now call Boyle s Law—the first Ideal Gas Law. Why must all high school chemistry students learn this simple relationship In part, because Boyle s Law and the other gas laws helped to establish the reality of atoms and molecules over 150 years later. [Pg.210]

FIGURE 146. In Fig. 5 we see Robert Boyle s famous J tube used to demonstrate that PV = k (Boyle s Law). Air is trapped by mercury in the small arm of the J tube. As more mercury is added, the volume of the air decreases. (From New Experiments Physico-Mechanical. . . , 1662). [Pg.211]

Robert Boyle (1627-1691) studied the effect of changing the pressure of a gas on its volume at constant temperature. He measured the volume of a given quantity of gas at a given pressure, changed its pressure, and measured the volume again. He obtained data similar to the data shown in Table 12-1. After repeating the process many times with several different gases, he concluded that [Pg.174]

The term inversely proportional in the statement of Boyle s law 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 if the pressure goes up to 5 times its previous value, the volume goes down to 5 of its previous value. This relationship can be represented mathematically by any of the following  [Pg.175]

EXAMPLE 12.2. What is the value of constant for the sample of gas for which data are given in Table 12-1  [Pg.175]

For each case, multiplying the observed pressure by the volume gives the value 8.0 L atm. Therefore, the constant k is 8.0 L-atm. [Pg.175]

200 ml of a gas is present in a cylinder at a pressure of 760 torr. If the gas is compressed by using a piston to a pressure of 950 torr, calculate the final volume occupied by the gas. (Assume the temperature to be constant) [Pg.79]

This problem specifically tests your knowledge of Boyle s law. We know that PFis a constant, provided that the temperature is kept constant. Since the temperature is constant, we can readily apply Boyle s law. We can equate the initial and final stages of the system. and F represent the initial pressure and volume respectively. P and F represent, the final pressure and volume respectively. [Pg.79]

In 1787, Jacques Charles showed that gas expands to occupy a larger volume as the temperature increases. Volume can be plotted against the temperature as shown below  [Pg.80]

When the temperature is increased, the volume increases. Charles found that the volume of a gas is directly proportional to its absolute temperature, provided that the pressure is kept constant. So the volume and temperature have a linear relationship as represented by the graph. Charles s law can be mathematically expressed as follows  [Pg.80]

The volume-temperature graph shows that at zero volume, the corresponding temperature value is -273.15° C. This means that at -273.15° C, the volume occupied by the gas is zero. This temperature is unique, and scientists so far have not been able to devise a way to lower the temperature to -273.15° C. [Pg.81]

4 Given the initial volume (or pressure) and initial and final pressures (or volumes) of a fixed quantity of gas at constant temperature, calculate the final volume (or pressure). [Pg.108]

Within experimental error, PV is indeed a constant (Fig. 4.12[b], third column). [Pg.109]

Boyle s Law, which this experiment illustrates, states that for a fixed quantity of gas at constant temperature, pressure is inversely proportional to volume. Equation 4.13 is the usual mathematical statement of Boyle s Law. Since the product of P and V is constant, when one factor increases the other must decrease. This is what is meant by an inverse proportionality. Notice the difference between an inverse proportionality and the direct proportionality of the previous section, where both variables increase or decrease together. [Pg.109]

Assume constant temperatme and amount of gas. (a) If the final pressure is less than the initial pressure, how will the final volume compare with the initial volume (b) If the final volume is greater than the initial volume, how will the final pressure compare with the initial pressure  [Pg.109]

Go to http //now.brookscole.com/ cracolice3e and click Chemistry Interactive for the module Boyle s Law. [Pg.109]

FIGURE 9.7 Pushing down the piston in the piston-cylinder arrangement changes the pressure from to P2 and the volume from to V2. (From Kenkel, J., Kelter, P., and Hage, D., Chemistry An Industry-Based Introduction with CD-ROM, CRC Press, Boca Raton, FL, 2001. With Permission.) [Pg.225]

If we push the piston down further, such that P = Pj and V = Vj, then we get the following  [Pg.225]

The constants indicated in Equations 9.2 and 9.3 are the same number if the pressures and volumes were measured in the same units each time. Thus we have the new relationship given in Equation 9.4. [Pg.225]

A gas occupies a volume of 75.3 mL at a pressure of 708 torn What volume will this gas occupy at 758 torr if the temperature does not change  [Pg.226]

The temperature has not changed, so Boyle s law holds true. The initial pressure, P, is 708 torr the final pressure, Pj, is 758 torr and the initial volume, Vi, is 75.3 mL. We must calculate Vg. Solving forVg in Equation 9.4, we have the following  [Pg.226]


From Boyles Law, it is known that the pressure is directly proportional to the temperature, therefore, it was shown that the kinetic energy of the molecules related directly to the temperature of the gas. A simple thermodynamic relation holds for this ... [Pg.3]

Boyles Law states The volume of a gas is inversely proportional to its absolute pressure, at a constant temperature. PjVj — P2V2... [Pg.690]

Boyles law—The volume and pressure of a gas are inversely proportional if the temperature and amount are constant. [Pg.121]

Supercompressibility of Natural Cos All gases deviate from the simple gas laws to a varying extent. This deviation is called super-compressibility and must be taken into account in gas measurement, particularly at high line pressure. For example, since natural gas is more compressible under high pressure at ordinary temperatures than is called for by Boyles law, gas purchased at an elevated pressure gives a greater volume when the pressure is reduced than it would if the gas were ideal. [Pg.11]

Here P, and V, represent the original pressure and volume, respectively, and P2 and V2 represent the second pressure and volume. This relationship is known as Boyle s Law after the 17th-century scientist Robert Boyle (see Chapter 3) who first described it. Boyles Law, however, only holds true assuming that the temperature and number of gas particles remain the same. [Pg.584]

We can use these postulates to rationalize the various gas laws (Table 17.2). For Boyles Law, pressure decreases with increasing volume because the impact of gas particles against the walls of the container is spread out (diluted) over a greater area. For Charles s Law, volume increases with increasing temperatures because faster-moving particles demand more room. Similarly, for Avogadro s Law, volume increases with an increasing number of particles because more particles also demand more room. [Pg.587]

Boyles Law A gas law that describes the inverted relationship between the pressure of a gas and its volume. The smaller the volume, the greater the pressure. [Pg.602]

At a depth of around 10 meters the pressure has been doubled. According to Boyles Law, the volume of air inside of the glass will be halved, which means that the water level will have risen to about the halfway mark. [Pg.702]

PERFECT GAS. A perfect gas may be defined by the following two laws The Joule law the energy per mole, U, depends only on the temperature the Boyle law at constant temperature, the volume V7 occupied by a given number of moles of gas varies in inverse proportion to the pressure. [Pg.1223]

Throughout history there have been multiple versions of gas laws developed and named after many different people. Boyles Law (1662), Charles s Law (1802), and Avogadro s Law (1811) are a few examples. [Pg.37]

So, the temperature of the gas at which the value of PV remains constant, so that Boyles law is fully obeyed, is known as Boyle s temperature (Tb). [Pg.86]

If the temperature is less than Boyles temperature, the value of Z first decreases and then reaches a minimum value and finally as the pressure is gradually increased, the value of Z starts increasing. Different gases have different Boyle temperatures. For hydrogen and helium, Boyle temperatures are -80°C and -240°C, respectively. It means that at -80°C, hydrogen obeys Boyles law within a maximum range of pressure. [Pg.86]

One mole of gas in) has is volume (V) specified by temperature (T) and pressure (it) according to the Charles-Boyle law, and any change in either of these two variables results in a corresponding change in the other, so that the following equation is satisfied ... [Pg.41]

Now that you ve finished practising Boyles law problems, take a deep breath and relax. You have just illustrated Boyles law When you inhale, muscles in your torso expand your rib cage. The volume of your lungs increases. Since the pressure inside your lungs is decreased with the expansion in volume, outside air under higher pressure rushes in. [Pg.435]

Note that the product of the pressure and the volume for each point in Figure 13.1 is 10 atm-L. Boyles law can be expressed mathematically as follows. [Pg.443]

Water is always present in the production of namral gas in both the liquid and vapor phases. If water liquid is present, molecules at the surface tend to escape into the space above. These molecules become vapor and are free to mix with the other constiment gases in the stream. Ultimately, an equilibrium, or steady state of balance is attained when the rate of escape and rate of return into solution are equal. When this condition occurs, the gas is said to be saturated with water vapor. For any gas, this condition of balance or samration is directly proportional to the temperature (Boyles Law, Ti=V] as T2=V2). The greater the temperature of the carrier natural gas, the greater the volume of water that can be absorbed into solution. Conversely, as the temperature of a gas begins to drop, the kinetic energy of the fluid deeieases. As this happens, the water vapor begins to condense and return to the liquid phase. [Pg.223]

BOYLES LAW - If the temperature on a gas is constant, the volume is inversely proportional to the pressure. By formula - VP = ViPi... [Pg.30]


See other pages where Boyles’law is mentioned: [Pg.690]    [Pg.719]    [Pg.803]    [Pg.41]    [Pg.53]    [Pg.239]    [Pg.706]    [Pg.73]    [Pg.130]    [Pg.151]    [Pg.468]    [Pg.151]   
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See also in sourсe #XX -- [ Pg.37 ]

See also in sourсe #XX -- [ Pg.21 ]

See also in sourсe #XX -- [ Pg.144 ]

See also in sourсe #XX -- [ Pg.17 , Pg.228 , Pg.231 ]




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