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Universal Gas Law

Of course, you should be familiar with this equation (the Ideal Gas Law), where n is the molar concentration of solute, R is the universal gas law constant, and T is absolute temperature in °K. The permeate flow can be calculated from ... [Pg.364]

Physicians can nse hqnid nitrogen to freeze and destroy warts and other skin growths. Knowing the assumptions of the universal gas law, this should surprise you most because —... [Pg.28]

In the attempt to devise some truly universal gas law for high pressures, the idea of corresponding states was developed. Early experimenters found that at the critical... [Pg.268]

Earher we talked about vapour pressure as one reason wlty solvents can cause problems, but there is another thing which applies to all gases and vapours which you need to know. It is based on the Universal Gas Law. This says that, as the temperature of a gas rises, so does the pressure if you do not change the volume. So pressure will rise as temperature does in a closed drum. [Pg.354]

At least two measures of concentration for airborne gases and vapours are in common use and these can be interconverted by reference to the universal gas law which applies to either total or partial pressures. [Pg.280]

Law 3 The Universal Gas Law—pressure and volume are directly related to temperature. The hotter the fire, the higher the pressure it develops. Confining the pressure (like in a dead end or in a roof cavity) increases the pressure and leads to explosions. The only difference between a FIRE and an EXPLOSION is how HEAT IS CONFINED. [Pg.376]

Although ion transmission guides and ion traps both use the same universal physical laws to achieve control over ion behavior, the ways in which the laws are used are different, as are the objectives. The guides do not retain ions to gain control over their velocities and are used simply to transmit both slow and fast ions over a very wide range of gas pressures. Ion traps retain ions over a relatively long period of time so as to adjust their kinetic energies and thereby improve mass resolution. The so-called bath gas is used at carefully controlled pressures. [Pg.378]

Steam is the working fluid in most boiler operations and usually can be treated as an ideal gas that is, a gas that obeys the ideal gas law. This law states that the pressure (P) of a volume of gas (v) is equal to the product of the universal gas constant (R) and temperature (7). [Pg.7]

Calculate the mol fractions and concentration gradients of the two components at the mid-point of the film. Assume that the ideal gas law is applicable and that the Universal Gas Constant R = 8314 J/kmol K. [Pg.858]

According to the combined gas law, the volume of a given mass of gas can have any value, depending on its temperature and pressure. To compare the quantities of gas present in two different samples, it is useful to adopt a set of standard conditions of temperature and pressure. By universal agreement, the standard temperature is chosen as 273 K (0°C) and the standard pressure is chosen as exactly 1 atm (760torr). Together, these conditions are referred to as standard conditions or as standard temperature and pressure (STP). While there is nothing special about STP, some authors and some instructors find it convenient to use this short notation for this particular temperature and pressure. [Pg.189]

At very low pressure all gases obey the ideal gas law, PV = nRT, where P is the pressure, V is the volume and, T is the temperature. The gas constant, R, is a universal constant, and T is the absolute temperature in kelvin. A mixture of gases at sufficiently low pressure also behaves ideally... [Pg.84]

Boyle s and Charles s laws are convenient if you happen to find yourself in situations where only two factors change at a time. But the universe is rarely so well-behaved. What if pressure, temperature, and volume all change at the same time Are aspirin and a nap the only solution No. Enter the combined gas law ... [Pg.159]

One particularly powerful insight students gain from this assignment is the limitations of the van der Waals equation of state. Often in undergraduate chemistry courses, the van der Waals equation is presented as the universal correction to the ideal gas law, perhaps owing to its straightforwardness and the ease with which it can be understood. Recognizing its limitations leads students to consider other equations of state, where each expression has its own set of assumptions. While students are initially uneasy with the notion that the van der Waals equation has drawbacks and that decisions about which EOS to use depends on the system or context, this unease is not uncommon in the execution of real science. [Pg.201]

The constant R is called the gas constant and has the same value for all gases because R is independent of the identity of the gas, we say that it is a universal constant. The ideal gas law is an example of an equation of state, an expression showing how the pressure of a substance—in this case, a gas—is related to the temperature, volume, and amount of substance in the sample. [Pg.305]

Casiday, Rachel, and Regina Frey. Chemistry Behind Airbags. Gas Laws Save Lives. Department of Chemistry, Washington University in St. Louis. Available online. URL http //www. chemistry.wustl.edu/ edudev/LabTutorials/Airbags/airbags. html. Accessed Dec. 17, 2006. [Pg.101]


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See also in sourсe #XX -- [ Pg.376 ]




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