0
What else can I help you with?
Why is the boyles law applicable only the idealgases?
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
Which of the following properties minimizes the differences between an ideal gas and a real gas?
- Weak intermolecular forces -Low density
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).
A real gas differs from an ideal gas because the molecules of real gas have?
higher molecular volumes and exhibit intermolecular forces, such as van der Waals forces, that cause deviations from ideal gas behavior. These intermolecular forces affect the compressibility, volume, and pressure of a real gas, making it different from the assumptions of an ideal gas.
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.
Is krypton an ideal gas?
Krypton is not an ideal gas because it deviates from the ideal gas law at high pressures and low temperatures due to its intermolecular interactions. At standard conditions, krypton behaves closely to an ideal gas, but as conditions vary, its non-ideal characteristics become more pronounced.
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
How does a real gas behave most nearly like an ideal gas?
A real gas behaves most like an ideal gas when it is at low pressure and high temperature.
At what conditions does a real gas behave most like an ideal gas?
A real gas behaves most like an ideal gas at high temperatures and low pressures.
Why is the boyles law applicable only the idealgases?
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
Which of the following properties minimizes the differences between an ideal gas and a real gas?
- Weak intermolecular forces -Low density
Would a gas whose molecules were true geometric points obey the ideal gas law?
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
What characteristics make a gas non-ideal?
The gas molecules interact with one another
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.
In an ideal gas compared to a real gas at very high pressure occupies?
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
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).
Is real gas a gas?
A real gas is a type of gas that is different than an ideal gas. They have completely different interactions between their molecules.
