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Why is it that gases show ideal behaviour when volume occupied is large?
Wiki User
∙ 8y ago
In a large volume the intermolecular collisions are rare.
Wiki User
∙ 8y ago
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Do ideal gases have volume and intermolecular attractive forces?
true
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.
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.
According to the ideal gas laws what happens to the volume of a gas when the number of moles doubles?
The product PV remain constant in a closed system at constant temperature.
Would air ever have zero volume at absolute zero?
No - the ideal gas law is an approximation for ideal gases, it doesn't apply exactly for real gases. Deviations are greater at very small temperatures, or very high pressures.
Chlorine gas occupies a volume of 25.0 mL at 300 K What volume will it occupy at 600 K?
If pressure is kept constant, and we assume ideal gas behaviour for chlorine, then its volume at 600 K would be 50.0 ml. Charles law of gases states that the volume of a gas kept at constant pressure, varies directly proportional to its absolute temperature. Of course, this result is not completely exact since real gases tend to deviate from ideal behaviour. But at low pressures the result is usually a good approximation.
Do ideal gases have volume and intermolecular attractive forces?
true
For ideal gas force of attraction between molecules?
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.
State relation between mole fraction and Volume fraction?
For Ideal gases, mole fraction=volume fraction
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 volume occupied by a mole of an ideal gas if the pressure is 626mmHg and the temperature is 25.0C?
I suppose that the correct anwer is 29,7 L.
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.
According to the ideal gas laws what happens to the volume of a gas when the number of moles doubles?
The product PV remain constant in a closed system at constant temperature.
What is avagadro's law in science?
The volume of ideal gases, at the same temperature and pressure, have the same number of particles/molecule.
How does the ideal gas law relate to real gases?
Ideal gas law states that there are no inter molecular attractions between gas molecules and that ideal gas does not occupy space therefore having no volume. However, a real gas does have intermolecular attractions and does have a volume.
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.
Identify the gas law that is used to describe gas behavior under a specific set of circumstances.?
Charles' Law and other observations of gases are incorporated into the Ideal Gas Law. The Ideal Gas Law states that in an ideal gas the relationship between pressure, volume, temperature, and mass as PV = nRT, where P is pressure, V is volume, n is the number of moles (a measure of mass), R is the gas constant, and T is temperature. While this law specifically applies to ideal gases, most gases approximate the Ideal Gas Law under most conditions. Of particular note is the inclusion of density (mass and volume) and temperature, indicating a relationship between these three properties.The relationship between the pressure, volume, temperature, and amount of a gas ~APEX
