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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 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.
When do real gases act least like ideal gases?
Real gases act least like ideal gases under conditions of high pressure and low temperature, where the gas molecules are closer together and experience intermolecular forces that are not accounted for in the ideal gas law.
Why do real gases deviate from ideal behavior?
Real gases deviate from ideal behavior due to factors such as intermolecular forces, molecular volume, and pressure. These factors cause real gases to occupy more space and have interactions that differ from the assumptions of the ideal gas law.
Ideal gas law behavior of real gases under?
Real gases deviate from ideal gas behavior at high pressures and low temperatures due to interactions between gas molecules. These interactions cause deviations in volume and pressure from what would be expected based on the ideal gas law. At very high pressures or very low temperatures, these deviations become significant and the ideal gas law no longer accurately describes the system.
What At low temperatures and pressure how does the volume of a real gas compare with the volume of an ideal gas under the same conditions?
It is less
What is partial pressure of a gas in a mixtures of gases?
The partial pressure is the pressure exerted by just one gas in the mixture.
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.
Is it true that the pressure exerted by real gas is less than that of ideal gas for both the attractive and repulsive interactions among the gas molecules?
Yes, it can be less. One of the assumptions made by the concept of the "ideal gas" is that there are no attractions at all between representative particles of that gas (along with 100% elasticity in collisions and statistically random motion.) These things don't truly happen in real gases, however, which means that the overall pressure (represented by collisions by particles with the inside walls of the container) could be lower. This is because the attractions between particles (see intermolecular forces) slow them down a little bit, along with those collisions, which aren't really completely elastic. All these factors can result in a slight lowering of pressure in a real gas compared to 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.
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.
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 do real gases act least like ideal gases?
Real gases act least like ideal gases under conditions of high pressure and low temperature, where the gas molecules are closer together and experience intermolecular forces that are not accounted for in the ideal gas law.
Why do real gases deviate from ideal behavior?
Real gases deviate from ideal behavior due to factors such as intermolecular forces, molecular volume, and pressure. These factors cause real gases to occupy more space and have interactions that differ from the assumptions of the ideal gas law.
What would make a real gas as close to ideal as possible?
High temperature; low pressure.
Which of the following properties minimizes the differences between an ideal gas and a real gas?
- Weak intermolecular forces -Low density
Is hydrogen a ideal gas?
Hydrogen is close to an ideal gas under certain conditions, particularly at low pressure and high temperature. However, deviations from ideal behavior can occur at high pressure and low temperature due to intermolecular interactions and molecular size effects.
