When the pressure is low and the temperature is high the molecules have less inter particle forces of attraction thus more inter particle spaces, which is a characteristic of gases .Therefore it is an ideal situation for gases.
Helium is most likely to behave as an ideal gas when it is under conditions of low pressure and high temperature. Ideal gases follow the ideal gas law, which assumes the gas molecules have negligible volume and there are no intermolecular forces between them. At low pressure and high temperature, the molecules are far apart and moving quickly, closer to the assumptions of an ideal gas.
Gases are most soluble in water under conditions of low temperature and high pressure. Additionally, the solubility of gases in water is often influenced by the nature of the gas itself and its polarity.
A real gas displays the most ideal behavior under conditions of low pressure and high temperature. At these conditions, the gas molecules are far apart and have high kinetic energy, resulting in weak intermolecular forces and minimal deviations from ideal gas behavior.
No. It takes a combination of pressure and temperature to liquefy some gases. Hydrogen and helium were the last gases to be liquefied and that was with pressure and extremely low temperature.
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.
When the pressure is low and the temperature is high the molecules have less inter particle forces of attraction thus more inter particle spaces, which is a characteristic of gases .Therefore it is an ideal situation for gases.
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.
Yes, if the pressure is low.
Helium is most likely to behave as an ideal gas when it is under conditions of low pressure and high temperature. Ideal gases follow the ideal gas law, which assumes the gas molecules have negligible volume and there are no intermolecular forces between them. At low pressure and high temperature, the molecules are far apart and moving quickly, closer to the assumptions of an ideal gas.
Gases deviate from ideal behavior at high pressure because the molecules are closer together, leading to stronger intermolecular forces that affect their behavior.
Gases are most soluble in water under conditions of low temperature and high pressure. Additionally, the solubility of gases in water is often influenced by the nature of the gas itself and its polarity.
Real gases behave most like ideal gases under conditions of low pressure and high temperature. At low pressures, the volume of gas molecules is significant compared to the volume of the container, and at high temperatures, intermolecular forces are minimized, allowing the gas molecules to behave more independently.
Oxygen gas behaves least like an ideal gas at low temperatures and high pressures. At low temperatures, the gas molecules move more slowly and can interact more with each other, deviating from ideal gas behavior. At high pressures, the gas molecules are closer together and experience stronger intermolecular forces, leading to less ideal behavior.
Real gases behave most like ideal gases at high temperatures and low pressures.CASE 1 :- (At Higher Temperatures)when the temperature is high the kinetic energy of molecules increases and the intermolecular attractions among the atoms decreases.The volume of the gas molecules become negligible compared to volume of the vessel. therefore the real gases act like ideal At Higher Temperatures.CASE 2 :- (At Lower Temperatures)At low temperatures volume of the container is larger. therefore intermolecular attractive forces are negligible and the volume of the particles also become negligible compared with the volume of the vessel.therefore the real gases act like ideal At Lower Temperatures.
High pressure, and low temperature.High pressure, and low temperature.High pressure, and low temperature.High pressure, and low temperature.
For gases, the most ideal conditions are low pressure (p), high temperature (T), and low molar volume (V/n). This is described by the ideal gas law equation, PV = nRT, where R is the ideal gas constant. These conditions ensure that gas molecules are far apart from each other and exhibit ideal behavior.