0
What else can I help you with?
Why hydrogen and helium can not be liquefied?
Hydrogen and helium have low boiling points, which are near absolute zero. Achieving temperatures this low is extremely challenging and energy-intensive, making it difficult to liquefy these gases. Additionally, at such low temperatures, the materials used to contain the gases would become brittle and may fail.
Why is butane gas not an ideal gas?
Butane gas is not an ideal gas because it exhibits some deviation from the ideal gas law at high pressures and low temperatures. This is due to the intermolecular forces present in butane molecules that influence their behavior. Additionally, butane gas can liquefy at relatively low temperatures, further deviating from ideal gas behavior.
How do gases behave under different pressures and different temperatures?
Gases behave differently at different pressures and temperatures. At low pressures, gases expand to fill the available space. At high pressures, gases become more compact. At low temperatures, gases condense into liquids or solids. At high temperatures, gases expand and exert greater pressure.
Which gas is most difficult to liquefy?
Helium is the gas that is most difficult to liquefy because it remains in a gaseous state even at extremely low temperatures. Its low boiling point and weak intermolecular forces make it challenging to convert into a liquid state.
Why gas law does not obey high pressure to low temperature?
Gas laws, such as Boyle's and Charles's laws, assume ideal behavior of gases, which breaks down at high pressures and low temperatures. Under these conditions, intermolecular forces become significant, and gas particles are forced closer together, deviating from ideal gas behavior. Additionally, low temperatures can cause gases to condense into liquids, further invalidating the assumptions of the gas laws. Thus, real gases do not conform to these laws under such extreme conditions.
When do gases deviate from ideal behavior?
Gases deviate from ideal behavior at high pressures and low temperatures.
Do real gases behave like ideal gases except at very high temperatures?
Gases behave most ideally at low pressure and high temperatures. At low pressures, the average distance of separation among atoms or molecules is greatest, minimizing interactive forces. At high temperatures, the atoms and molecules are in rapid motion and are able to overcome interactive forces more easily.
Why hydrogen and helium can not be liquefied?
Hydrogen and helium have low boiling points, which are near absolute zero. Achieving temperatures this low is extremely challenging and energy-intensive, making it difficult to liquefy these gases. Additionally, at such low temperatures, the materials used to contain the gases would become brittle and may fail.
Why do real gases deviate from the ideal gases laws at low temperatures?
Ideal gases theoretically have no mass, they are single points. Normally the small size (in comparison to the large space between them) of non-ideal gasses is insignificant, however at low temperatures when kinetic energy and the space between particles is low this mass has significant effects.
Why is butane gas not an ideal gas?
Butane gas is not an ideal gas because it exhibits some deviation from the ideal gas law at high pressures and low temperatures. This is due to the intermolecular forces present in butane molecules that influence their behavior. Additionally, butane gas can liquefy at relatively low temperatures, further deviating from ideal gas behavior.
At what temperature does a real gas obey the ideal gas laws over a wide range of pressure?
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.
How do we liquefy gases?
Gases can be liquefied by applying pressure and reducing the temperature below their critical points. This causes the gas molecules to come closer together and form a liquid. This process is typically done in a container that can withstand high pressure and low temperatures.
How do gases condense?
Gases are condensed at low temperatures.
Why do gases behave most ideally?
is it true the space between gas particles becomes very large
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.
Which conditions of p t and n respectively are most ideal for gases?
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.
Which description applies to real gases rather than ideal gases?
Real gases deviate from ideal behavior at high pressures and low temperatures due to interactions between gas molecules. Real gases have non-zero volumes and experience intermolecular forces, unlike ideal gases which have zero volume and do not interact with each other.
