0
the ideal gas law describes that the behavior of real gases under all conditions of temperature and pressure.
Wiki User
∙ 12y ago
Add your answer:
Earn +20 pts
State 2 factors that van Der Waals proposed to explain why real gases deviate from ideal behavior?
nuawgfaw
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
Do real gases follow the ideal gas equation?
The gas which obeyed the gas laws at all conditions of temperature and pressure would be called an ideal gas. They don't actually exist. Real gases obey the gas laws approximately under moderate conditions. Some other points of distinction that can be considered are:Ideal gases are incompressible, non-viscous & non-turbulent.Real gases are compressible, viscous & turbulent.
Which description applies to real gases rather than ideal gases?
the ratio of PV to nRT is always 1.
What are the deviations of the ideal gas accounted for in the equations of state of real gass?
An ideal gas, by definition, follows the Ideal Gas Law, which states PV=nRT. Any behavior for which that equation does not hold is considered non-ideal. What then are the causes of non-ideal behavior? The Ideal Gas Law doesn't work for many gases (in other words, many gas are not actually ideal) because the Gas Law makes two assumptions, that in certain conditions break down. Assumption #1 is that there are no interactions between atoms/molecules in the gas phase. In this model, there are no attractive or repulsive forces between two neighboring atoms/molecules in the gas phase. This is not always correct, and especially at very low temperatures, gases tend to condense, and so attractive forces between them start to be significant. Attractive forces tend to make the measured pressure lower than it is predicted to be. Assumption #2 is that the volume of the container holding the gas is infinitely larger than the volume taken up by the gas molecules themselves. In other words, it assumes that molecules have zero volume, which is of course not true. This assumption breaks down significantly at very high pressures, where the volume taken up by the gas is significant compared to the volume of the container. To correct for this, the molecular volume taken up by the gas is subtracted from the volume of the empty container. Therefore, there are significant deviations from the Ideal Gas Law at high pressures or very low temperatures. The actual amount of deviation depends on the molecules individual properties. H2 gas or He gas are both very "ideal" gases under most conditions. However, H2O, with strong intermolecular attractive forces, or SO2 (a fairly large molecule also with strong intermolecular forces) do not obey the Ideal Gas Law under most conditions.
What is an imaginary gas that conforms perfectly to the kinetic molecular theory callled?
That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.That's called an "ideal gas". The behavior of real gases is quite similar to an ideal gas, except when the pressure is too high, or the temperature too low.
When does a real gas display the most ideal behavior?
This is a gas having a high concentration.
How can a real gas be made to approach being an ideal gas?
Real gases approach ideal behavior at high temperature and low pressure. In this Condition gases occupy a large volume and molecules are far apart so volume of gas molecules are negligible and intermolecular force of attraction(responsible for non ideal behavior) become low. So gases approach ideal behavior.
Why real gases deaviat from ideal behaviou?
It is assumed that Ideal Gases have negligible intermolecular forces and that the molecules' actualphysical volume is negligible. Real Gases have the molecules closer together so that intermolecular forces and molecules' physical volumes are no longer negligible. High pressures and low temperatures tend to produce deviation from Ideal Gas Law and Ideal Gas behavior.
State 2 factors that van Der Waals proposed to explain why real gases deviate from ideal behavior?
nuawgfaw
Do real gases behave like ideal gases except at very high temperatures?
Gases behave most ideally at low pressure and high temperatures. At low pressures, the average distance of separation among atoms or molecules is greatest, minimizing interactive forces. At high temperatures, the atoms and molecules are in rapid motion and are able to overcome interactive forces more easily.
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
How does an ideal gas diff from a real gas?
Ideal gases are gases with negligible intermolecular forces and molecular volumes. Real gases have intermolecular forces and have definite volumes at room temperature and pressure (RTP).
What are real and ideal gases and are all real gases ideal?
Ideal gases can be explained by the Kinetic Molecular Theory: 1) no attraction between gas particles 2) volume of individual gas particles are essentially zero 3) occupy all space available 4) random motion 5) the average kinetic energy is directly proportional to Kelvin Real gases has volume and attraction exists between gas particles. No gas behaves entirely ideal. Real gases act most ideal when temperature is is high and at low pressure.
What is meant by the term 'ideal gas'?
An ideal gas is a theoretical gas composed of a set of randomly-moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law. At normal conditions such as standard temperature and pressure, most real gases behave qualitatively like an ideal gas. Many gases such as air, nitrogen, oxygen, hydrogen, noble gases, and some heavier gases like carbon dioxide can be treated like ideal gases within reasonable tolerances.
What is the difference between the Ideal Gas Law and Kinetic Molecular Theory?
KMT talks about the properties of real gases while ideal gas laws discuss only the ideal gases..
What is the significance of the real gas equation?
The real gas equation, also known as the Van der Waals equation, is significant because it accounts for the deviations from ideal gas behavior. It incorporates corrections for intermolecular forces and the volume occupied by gas molecules, which are neglected in the ideal gas equation. This equation is crucial for studying real gases at high pressures and low temperatures.
