<%= durationStr% <%= title% <%= tooltipContentBody% <%= title%. <%= durationStr% <%= tooltipContentBody%. El vocho es un F.I 1994 el problema esque se acelera y desacelera solo, cuando esta parado y si vas despacio en segunda o tercera este empieza a tironearse por lo mismo que se acelera y desacelera solo.

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La solucion fue la siguiente este vocho en F.I 1994 los primeros modelos venian con generador no con alternador la solucion fue ponerlo a 6 grados de tiempo lo mas bajo pero dentro de los parametros. Esa es la solucion mas basica la completa seria cambiar a alternador y subir a 8 grados ahora si sus vochos son 1995 en adelante vienen con alternador y si hace eese problema jamas piensen que es la valvula ralenti o iak. Por que no lo es las posibles causas son las siguientes sensor de oxigeno, alternador malo, map o problemas electricos de origen en el alternador. Y estos general problemas de mala mezcla en combustible y por consecuencia gasto alto de combustible. Gas phase particles (, or ) move around freely in the absence of an applied. Gas is one of (the others being and ). Near, a substance exists as a.

As heat is added to this substance it melts into a at its (see ), boils into a gas at its, and if heated high enough would enter a state in which the are so energized that they leave their parent atoms from within the gas. A pure gas may be made up of individual atoms (e.g. A or atomic gas like ), molecules made from one type of atom (e.g.

), or molecules made from a variety of atoms (e.g. A gas would contain a variety of pure gases much like the.

What distinguishes a gas from liquids and solids is the vast separation of the individual gas particles. This separation usually makes a colorless gas invisible to the human observer. The interaction of gas particles in the presence of electric and are considered negligible as indicated by the constant velocity vectors in the image. The gaseous state of matter is found between the liquid and plasma states, the latter of which provides the upper temperature boundary for gases.

Bounding the lower end of the scale lie degenerative quantum gases which are gaining increased attention these days. High-density atomic gases super cooled to incredibly low temperatures are classified by their statistical behavior as either a or a. For a comprehensive listing of these exotic states of matter see.

Drifting particles provide clues to the movement of the surrounding gas. As most gases are difficult to observe directly with our senses, they are described through the use of four or characteristics:, (chemists group them by ) and. These four characteristics were repeatedly observed by scientists such as, and for a variety of gases in various settings. Their detailed studies ultimately led to a mathematical relationship among these properties expressed by the (see simplified models section below). Gas particles are widely separated from one another, and as such are not as strongly intermolecularly bonded to the same degree as liquids or solids.

These result from electrostatic interactions between each gas particle. Like charged areas of different gas particles repel, while oppositely charged regions of different gas particles attract one another; gases that contain permanently charged are known as.

Gaseous compounds with bonds contain permanent charge imbalances and so experience relatively strong intermolecular forces, although the molecule while the compound's net charge remains neutral. Transient, randomly-induced charges exist across non-polar of molecules and electrostatic interactions caused by them are referred to as. The interaction of these intermolecular forces varies within a substance which determines many of the physical properties unique to each gas. A quick comparison of boiling points for compounds formed by ionic and covalent bonds leads us to this conclusion. The drifting smoke particles in the image provides some insight into low pressure gas behavior.

Compared to the other states of matter, gases have an incredibly low and. And influence the particles within a certain volume.

This variation in particle separation and speed is referred to as compressibility. This particle separation and size influences optical properties of gases as can be found in the following. Finally, gas particles spread apart or in order to homogeneously distribute themselves throughout any container.

Shuttle imagery of re-entry phase. When observing a gas, it is typical to specify a frame of reference. A larger length scale corresponds to a or global point of view of the gas.

This region (referred to as a volume) must be sufficient in size to contain a large sampling of gas particles. The resulting statistical analysis of this sample size produces the 'average' behavior (i.e.

Velocity, temperature or pressure) of all the gas particles within the region. By way of contrast, a smaller length scale corresponds to a or particle point of view. From this global vantage point, the gas characteristics measured are either in terms of the gas particles themselves (velocity, pressure, or temperature) or their surroundings (volume).

By way of example, Robert Boyle studied for a small portion of his career. One of his experiments related the properties of pressure and volume of a gas. His experiment used a J-tube which looks like a in the shape of the letter J. Boyle trapped an gas in the closed end of the test tube with a column of, thereby locking the number of particles and temperature. He observed that when the pressure was increased on the gas, by adding more mercury to the column, the trapped gas volume decreased.

Mathematicians describe this situation as an relationship. Furthermore, when Boyle multiplied the pressure and volume of each observation, the was always the same, a constant. This relationship held true for every gas that Boyle observed leading to the law, (PV=k), named to honor his work in this field of study. There are many math tools to choose from when analyzing gas properties. As gases are subjected to extreme conditions, the math tools become a bit more complex, from the (inviscid flow) to the that fully account for viscous effects.

These equations are tailored to meet the unique conditions of the gas system in question. Boyle's lab equipment allowed the use of to obtain his analytical results. His results were possible because he was studying gases in relatively low pressure situations where they behaved in an 'ideal' manner. These ideal relationships enable safety calculations for a variety of flight conditions on the materials in use. The high technology equipment in use today was designed to help us safely explore the more exotic operating environments where the gases no longer behave in an 'ideal' manner. This advanced math, to include and, makes possible the solution to such complex dynamic situations as space vehicle reentry.

One such example might be the analysis of the image depicting space shuttle reentry to ensure the material properties under this loading condition are not exceeded. It is safe to say that in this flight regime, the gas is no longer behaving ideally. Main article: The symbol used to represent pressure in equations is 'p' or 'P' with SI units of. When describing a container of gas, the term (or absolute pressure) refers to the average force the gas exerts on the surface area of the container.

Within this volume, it is sometimes easier to visualize the gas particles moving in straight lines until they collide with the container (see diagram at top of the article). The force imparted by a gas particle into the container during this collision is the change in of the particle. As a reminder from, momentum, by definition, is the product of mass and velocity. Notice that during a collision only the normal component of velocity changes.

A particle traveling parallel to the wall never changes its momentum. So the average force on a surface must be the average change in from all of these gas particle collisions.

To be more precise, pressure is the sum of all the of force exerted by the particles impacting the walls of the container divided by the surface area of the wall. The image 'Pressurized gases' depicts gas pressure and temperature spikes used in the entertainment industry. Main article: The symbol used to represent temperature in equations is T with SI units of. The speed of a gas particle is proportional to its.

The volume of the balloon in the video shrinks when the trapped gas particles slow down with the addition of extremely cold nitrogen. The temperature of any is related to the motions of the particles (molecules and atoms) which make up the gas system. In, temperature is the measure of the average kinetic energy stored in a particle. The methods of storing this energy are dictated by the of the particle itself. Kinetic energy added ( process) to gas particles by way of collisions produces linear, rotational, and vibrational motion as well.

By contrast, a molecule in a solid can only increase its vibration modes with the addition of heat as the lattice crystal structure prevents both linear and rotational motions. These heated gas molecules have a greater speed range which constantly varies due to constant collisions with other particles. The speed range can be described by the. Use of this distribution implies near for the system of particles being considered.

See also: The symbol used to represent volume in equations is 'V' with SI units of cubic meters. When performing a analysis, it is typical to speak of. Properties which depend on the amount of gas (either by mass or volume) are called extensive properties, while properties that do not depend on the amount of gas are called intensive properties.

Specific volume is an example of an intensive property because it is the ratio of volume occupied by a unit of mass of a gas that is identical throughout a system at equilibrium. 1000 atoms of as a gas occupy the same space as any other 1000 atoms for any given temperature and pressure. This concept is easier to visualize for solids such as which are compared to gases.

When the seat ejection is initiated in the rocket sled image the specific volume increases with the expanding gases, while mass is conserved. Since a gas fills any container in which it is placed, volume is an extensive property. Main article: The symbol used to represent density in equations is ρ (pronounced rho) with SI units of kilograms per cubic meter. This term is the of specific volume.

Since gas molecules can move freely within a container, their mass is normally characterized by density. Density is the mass per volume of a substance or simply, the inverse of specific volume. For gases, the density can vary over a wide range because the particles are free to move closer together when constrained by pressure or volume or both. This variation of density is referred to as. Like pressure and temperature, density is a of a gas and the change in density during any process is governed by the laws of thermodynamics. For a, the density is the same throughout the entire container. Density is therefore a; it is a simple physical quantity that has a magnitude but no direction associated with it.

It can be shown by kinetic theory that the density is inversely proportional to the size of the container in which a fixed mass of gas is confined. In this case of a fixed mass, the density decreases as the volume increases. If one could observe a gas under a powerful microscope, one would see a collection of particles (molecules, atoms, ions, electrons, etc.) without any definite shape or volume that are in more or less random motion. These neutral gas particles only change direction when they collide with another particle or the sides of the container. By stipulating that these collisions are perfectly elastic, this substance is transformed from a real to an ideal gas. This particle or view of a gas is described by the.

All of the assumptions behind this theory can be found in the postulates section of. Main article: Kinetic theory provides insight into the macroscopic properties of gases by considering their molecular composition and motion. Starting with the definitions of and, one can use the and geometric relationships of a cube to relate macro system properties of temperature and pressure to the microscopic property of kinetic energy per molecule. The theory provides averaged values for these two properties.

The theory also explains how the gas system responds to change. For example, as a gas is heated from absolute zero, when it is (in theory) perfectly still, its (temperature) is increased. As a gas is heated, the particles speed up and its temperature rise. This results in greater numbers of collisions with the container sides each second due to the higher particle speeds associated with elevated temperatures. As the number of collisions (per unit time) increase on the surface area of the container, the pressure increases in a proportional manner. Main article: Brownian motion is the mathematical model used to describe the random movement of particles suspended in a fluid. The gas particle animation, using pink and green particles, illustrates how this behavior results in the spreading out of gases.

These events are also described. Since it is at the limit of (or beyond) current technology to observe individual gas particles (atoms or molecules), only theoretical calculations give suggestions as to how they move, but their motion is different from Brownian Motion. The reason is that Brownian Motion involves a smooth drag due to the frictional force of many gas molecules, punctuated by violent collisions of an individual (or several) gas molecule(s) with the particle. The particle (generally consisting of millions or billions of atoms) thus moves in a jagged course, yet not so jagged as would be expected if an individual gas molecule was examined. Main articles: and As discussed earlier, momentary attractions (or repulsions) between particles have an effect on. In, the name given to these intermolecular forces is van der Waals force.

These forces play a key role in determining of a gas such as and (see physical characteristics section). Ignoring these forces in certain conditions (see ) allows a to be treated like an. This assumption allows the use of which greatly simplifies the path to a solution.

Proper use of these gas relationships requires us to take one more look at the (KMT). When these gas particles possess a magnetic charge or they gradually influence one another as the spacing between them is reduced (the hydrogen bond model illustrates one example).

In the absence of any charge, at some point when the spacing between gas particles is greatly reduced they can no longer avoid collisions between themselves at normal gas temperatures found in a lab. Another case for increased collisions among gas particles would include a fixed volume of gas, which upon heating would contain very fast particles.

What this means to us is that these ideal equations provide reasonable results except for extremely high pressure compressible or high temperature ionized conditions. Notice that all of these excepted conditions allow energy transfer to take place within the gas system. The absence of these internal transfers is what is referred to as ideal conditions (perfect – or well behaved) in which the energy exchange occurs only at the boundaries of the system. Real gases experience some of these collisions and intermolecular forces. When these collisions are statistically negligible incompressible, results from these ideal equations are still valid. At the other end of the spectrum, when the gas particles are compressed into close proximity they behave more like a liquid, and hence another connection to.

Main article: An equation of state (for gases) is a mathematical model used to roughly describe or predict the state properties of a gas. At present, there is no single equation of state that accurately predicts the properties of all gases under all conditions. Therefore, a number of much more accurate equations of state have been developed for gases in specific temperature and pressure ranges. The 'gas models' that are most widely discussed are 'perfect gas', 'ideal gas' and 'real gas'. Each of these models has its own set of assumptions to facilitate the analysis of a given thermodynamic system.

Each successive model expands the temperature range of coverage to which it applies. The image of first powered flight at illustrates one example on the successful application of these relationships in 1903. More recent examples include the 2009 maiden flights of the first solar powered aircraft, the, and the first commercial airliner to be constructed primarily from, the. Main article: The for an ideal or perfect gas is the and reads Failed to parse (Missing texvc executable; please see math/README to configure.): PV=nRT, where P is the pressure, V is the volume, n is amount of gas (in mol units), R is the, 8.314 J/(mol K), and T is the temperature.

Written this way, it is sometimes called the 'chemist's version', since it emphasizes the number of molecules n. It can also be written as Failed to parse (Missing texvc executable; please see math/README to configure.): PV= rho Rs T, where Failed to parse (Missing texvc executable; please see math/README to configure.): Rs is the specific gas constant for a particular gas, in units J/(kg K). This notation is the 'gas dynamicist's' version, which is more practical in modeling of gas flows involving acceleration without chemical reactions. The ideal gas law does not make an assumption about the specific heat of a gas. In the most general case, the specific heat is a function of both temperature and pressure. If the pressure-dependence is neglected (and possibly the temperature-dependence as well) in a particular application, sometimes the gas is said to be a, although the exact assumptions may vary depending on the author and/or field of science.

For an ideal gas, the ideal gas law applies without restrictions on the specific heat. An ideal gas is a simplified 'real gas' with the assumption that the Z is set to 1 meaning that this pneumatic ratio remains constant. A compressibility factor of one also requires the four state variables to follow the.

This approximation is more suitable for applications in engineering although simpler models can be used to produce a 'ball-park' range as to where the real solution should lie. An example where the 'ideal gas approximation' would be suitable would be inside a of a. It may also be useful to keep the elementary reactions and chemical dissociations for calculating. Main article: Each one of the assumptions listed below adds to the complexity of the problem's solution. As the density of a gas increases with pressure rises, the intermolecular forces play a more substantial role in gas behavior which results in the ideal gas law no longer providing 'reasonable' results. At the upper end of the engine temperature ranges (e.g. Combustor sections – 1300 K), the complex fuel particles absorb internal energy by means of rotations and vibrations that cause their specific heats to vary from those of diatomic molecules and noble gases.

At more than double that temperature, electronic excitation and dissociation of the gas particles begins to occur causing the pressure to adjust to a greater number of particles (transition from gas to ). Finally, all of the thermodynamic processes were presumed to describe uniform gases whose velocities varied according to a fixed distribution. Using a non-equilibrium situation implies the flow field must be characterized in some manner to enable a solution.

One of the first attempts to expand the boundaries of the ideal gas law was to include coverage for different by adjusting the equation to read pV n = constant and then varying the n through different values such as the, γ. Real gas effects include those adjustments made to account for a greater range of gas behavior:. ( Z allowed to vary from 1.0). Variable (specific heats vary with temperature). Van der Waals forces (related to compressibility, can substitute other equations of state). Issues with molecular and with variable composition.

For most applications, such a detailed analysis is excessive. Examples where 'Real Gas effects' would have a significant impact would be on the where extremely high temperatures and pressures are present or the gases produced during geological events as in the image of the 1990 eruption of. Main article: Boyle's Law was perhaps the first expression of an equation of state. In 1662 performed a series of experiments employing a J-shaped glass tube, which was sealed on one end. Mercury was added to the tube, trapping a fixed quantity of air in the short, sealed end of the tube. Then the volume of gas was carefully measured as additional mercury was added to the tube. The pressure of the gas could be determined by the difference between the mercury level in the short end of the tube and that in the long, open end.

Through these experiments, Boyle noted that the gas volume varied inversely with the pressure. The image of Boyle's Equipment shows some of the exotic tools used by Boyle during his study of gases. Boyle's Law – describes a gas in which the number of particles and Temperature are constant. PV = constant in this situation constant = nRT from the ideal gas law. Main articles: and In 1787, the French physicist and balloon pioneer, found that oxygen, nitrogen, hydrogen, carbon dioxide, and air expand to the same extent over the same 80 kelvin interval.

In 1802, published results of similar, though more extensive experiments, indicating a linear relationship between volume and temperature. Gay-Lussac credited Charle's earlier work by naming the law in his honor. In the absence of this linkage, Dalton could have been in contention for this honor for his previously published work on partial pressures. Law of Volumes – Both Charles and Gay-Lussac played a role in developing this relationship.

V/T = constant – notice that constant = nR/P from the ideal gas law. Main article: In 1811, Amedeo Avogadro verified that equal volumes of pure gases contain the same number of particles. His theory was not generally accepted until 1858 when another Italian chemist Stanislao Cannizzaro was able to explain non-ideal exceptions. For his work with gases a century prior, the number that bears his name represents the number of atoms found in 12 grams of elemental carbon-12 (6.022×10 23 mol −1). This specific number of gas particles, at standard temperature and pressure (ideal gas law) occupies 22.40 liters, which is referred to as the. Avogadro's Law – describes a gas in a container in which the pressure and temperature are constant.

The simplified form for the ideal gas law follows:. V/n = constant – notice that constant = RT/P from the ideal gas law. Main article: In 1801, published the Law of Partial Pressures from his work with ideal gas law relationship: The pressure of a mixture of gases is equal to the sum of the pressures of all of the constituent gases alone. Mathematically, this can be represented for n species as: Pressure total = Pressure 1 + Pressure 2 +.

+ Pressure n The image of Dalton's journal depicts symbology he used as shorthand to record the path he followed. Among his key journal observations upon mixing unreactive 'elastic fluids' (gases) were the following.:. Unlike liquids, heavier gases did not drift to the bottom upon mixing. Gas particle identity played no role in determining final pressure (they behaved as if their size was negligible). Main article: Viscosity, a physical property, is a measure of how well adjacent molecules stick to one another. A solid can withstand a shearing force due to the strength of these sticky intermolecular forces.

A fluid will continuously deform when subjected to a similar load. While a gas has a lower value of viscosity than a liquid, it is still an observable property. If gases had no viscosity, then they would not stick to the surface of a wing and form a boundary layer. A study of the in the image reveals that the gas particles stick to one another (see Boundary layer section). Main article: Particles will, in effect, 'stick' to the surface of an object moving through it. This layer of particles is called the boundary layer.

At the surface of the object, it is essentially static due to the friction of the surface. The object, with its boundary layer is effectively the new shape of the object that the rest of the molecules 'see' as the object approaches. This boundary layer can separate from the surface, essentially creating a new surface and completely changing the flow path.

The classical example of this is a. The delta wing image clearly shows the boundary layer thickening as the gas flows from right to left along the leading edge. Main article: As the total number of degrees of freedom approaches infinity, the system will be found in the that corresponds to the highest.

In order to illustrate this principle, observe the skin temperature of a frozen metal bar. Using a thermal image of the skin temperature, note the temperature distribution on the surface. This initial observation of temperature represents a '.' At some future time, a second observation of the skin temperature produces a second microstate. By continuing this observation process, it is possible to produce a series of microstates that illustrate the thermal history of the bar's surface. Characterization of this historical series of microstates is possible by choosing the macrostate that successfully classifies them all into a single grouping. Main article: When energy transfer ceases from a system, this condition is referred to as thermodynamic equilibrium.

Usually this condition implies the system and surroundings are at the same temperature so that heat no longer transfers between them. It also implies that external forces are balanced (volume does not change), and all chemical reactions within the system are complete. The timeline varies for these events depending on the system in question.

A container of ice allowed to melt at room temperature takes hours, while in semiconductors the heat transfer that occurs in the device transition from an on to off state could be on the order of a few nanoseconds. This early 20th century discussion infers what is regarded as the plasma state. See page 137 of American Chemical Society, Faraday Society, Chemical Society (Great Britain) The Journal of physical chemistry, Volume 11 Cornell (1907). The work by T. Zelevinski provides another link to latest research about Strontium in this new field of study. See Tanya Zelevinsky (2009). Physics 2: 94.

for links material on the see. 4 November 2009. Harper, Douglas. The authors make the connection between molecular forces of metals and their corresponding physical properties. By extension, this concept would apply to gases as well, though not universally.

Cornell (1907) pp. One noticeable exception to this physical property connection is conductivity which varies depending on the state of matter (ionic compounds in water) as described by in the 1833 when he noted that ice does not conduct a current. See page 45 of John Tyndall's Faraday as a Discoverer (1868). Hutchinson (2008). Anderson, p.501. J.

Clerk Maxwell (1904). Theory of Heat. Mineola: Dover Publications. See pages 137–8 of Society, Cornell (1907).

Kenneth Wark (1977). Thermodynamics (3 ed.). For assumptions of Kinetic Theory see McPherson, pp.60–61. Anderson, pp. 289–291. John, p.205. John, pp.

247–56. McPherson, pp.52–55. McPherson, pp.55–60. John P. Millington (1906). Pp. 72, 77–78. Fundamentals of Aerodynamics.

McGraw-Hill Higher Education. John, James (1984).

Gas Dynamics. Allyn and Bacon. McPherson, William and Henderson, William (1917). An Elementary study of chemistry.

Philip Hill and Carl Peterson. Mechanics and Thermodynamics of Propulsion: Second Edition Addison-Wesley, 1992. National Aeronautics and Space Administration (NASA). Accessed February, 2008. Georgia State University. Accessed February, 2008.

Antony Lewis. Accessed February, 2008. Northwestern Michigan College. Accessed February, 2008.

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