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In an ideal gas there is no attarcation between molecules. There is no such thing as an ideal gas it is a model that approximates the behaviour of real gases.
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What best describes the molecules of an ideal gas?
no volume, no intermolecular force of attraction, perfectly elastic collisions
What are the characteristics of an ideal gas?
1. Elastic Collision (no loss of kinetic energy when molecules hit) 2. Constant, rapid, and random motion 3. No attraction or repulsion between molecules (electromagnetic forces don't effect the collisions)
Are there forces of attraction between the particles in a gas?
No they dont because the kinetic theory of gases made us know that the intermolecular forces between them are weak and they are independent. They dont tend to attract because of the level of disorderliness at increase in temperature and pressure.
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.
Is ideal gas one whose particles take up space?
An ideal gas is a theoritical gas consisting of randomly moving particles.The kinetic theory of ideal gases makes 5 main assumptions:The size of molecules is negligible compared with the mean intermolecular distance (i.e. they are widely spaced molecules).Molecules move with different speeds and in random directions.Standard laws of motion apply.Collisions between molecules are elastic. Translational kinetic energy is not converted into other forms of energy.There are no attractive intermolecular forces between molecules except during collision.
What best describes the molecules of an ideal gas?
no volume, no intermolecular force of attraction, perfectly elastic collisions
Which gas of the following will have the greatest deviation from ideal behavior H2 F2 Br2 and Cl2?
The two factor Van de Waals gave as correction for real molecules instead of the ideal gas, are the size of the molecule, and the amount of attraction between the molecules. The larger the size of the molecule for the greater the deviation from an ideal gas, clearly bromine wins here since it has the biggest size of its atom. The amount of attraction between molecules is directly proportional to the boiling point of the liquid made from those molecules, and again bromine wins here since its has the highest boiling point. So bromine has the greatest deviation from ideal gas behaviour.
What are the characteristics of an ideal gas?
1. Elastic Collision (no loss of kinetic energy when molecules hit) 2. Constant, rapid, and random motion 3. No attraction or repulsion between molecules (electromagnetic forces don't effect the collisions)
A real gas differs from an ideal gas because the molecules of real gas have?
The molecules of real gas have some volume and some attraction for each other.
What are two characteristics of an ideal gas that are not true of a real gas?
they have no volume and their molecular force of attraction is negligible
Hydrogen and helium are ideal gases at room temperature and ordinary pressure but sulfur dioxide is not an ideal gas?
H2 and He are ideal at room temperature because room temperature is very high for both of them so at high temperature gasses bahaves ideally due to the small force of attraction but in case of SO2 and CL2 room temperature is not so high for them so they have greater force of attraction between them and thus behaves non-ideally .......!
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
Are there forces of attraction between the particles in a gas?
No they dont because the kinetic theory of gases made us know that the intermolecular forces between them are weak and they are independent. They dont tend to attract because of the level of disorderliness at increase in temperature and pressure.
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 happenes to the particels of a gas when there are fewer of them?
This is the ideal gas with no collisions between molecules..
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).
