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In all the fields of science (and also in economy, politics, moral, medicine, etc.) the ideal state is only a word. The ideal doesn't exist but it is very necessary to elaborate valid theories. In conclusion one can say that xenon is still a (quasi)ideal gas.
Xenon deviates from ideal gas behavior due to its relatively large atomic/molecular size and interactions between xenon atoms. At higher pressures and lower temperatures, these interactions become more significant, causing xenon to deviate from ideal gas behavior. These deviations are better described by the Van der Waals equation or other equations of state.
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What is the volume of 131.3 grams of xenon?
The volume of a gas like xenon can be calculated using the ideal gas law equation: PV = nRT. Given the mass of xenon, you would first need to convert it to moles using the molar mass of xenon (131.3 g/mol). Then, using the ideal gas constant (R) and the temperature and pressure of the gas, you can calculate the volume.
What 2 gases on the periodic table behave like ideal gases?
Two gases on the periodic table that behave like ideal gases are helium (He) and neon (Ne). Ideal gases follow the ideal gas law, which assumes that the gas particles are point masses and do not interact with each other. Helium and neon have low atomic masses and weak intermolecular forces, making their behavior close to ideal in most conditions.
Under which conditions does a real gas behave most like an ideal gas?
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.
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
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.
What is the pH of xenon?
Xenon is a noble gas and does not exhibit typical pH properties like acids or bases. Therefore, xenon does not have a pH value.
What is the volume of 131.3 grams of xenon?
The volume of a gas like xenon can be calculated using the ideal gas law equation: PV = nRT. Given the mass of xenon, you would first need to convert it to moles using the molar mass of xenon (131.3 g/mol). Then, using the ideal gas constant (R) and the temperature and pressure of the gas, you can calculate the volume.
What is the truth about a real gas to behave like an ideal gas?
CO2 can behave like an ideal gas, but is not an ideal gas. Depending on the temperature and amount of pressure applied, virtually all gasses can behave as ideal gasses. The ideal gas equation can be used on CO2 as a good approximation. (P = nRT/(V-nb) - an^2/V^2)
What 2 gases on the periodic table behave like ideal gases?
Two gases on the periodic table that behave like ideal gases are helium (He) and neon (Ne). Ideal gases follow the ideal gas law, which assumes that the gas particles are point masses and do not interact with each other. Helium and neon have low atomic masses and weak intermolecular forces, making their behavior close to ideal in most conditions.
What gas is likely to behave as an ideal gas when subjected to high temperature and low pressure?
Helium
How can a real gas be made to approach being an ideal gas?
A real gas can approach being an ideal gas by decreasing its pressure and increasing its temperature. At low pressures or high temperatures, the interactions between gas molecules become less significant, causing the gas to behave more like an ideal gas. Additionally, using larger volumes can also help minimize intermolecular interactions and make a real gas behave more like an ideal gas.
What is meant by the term 'ideal gas'?
An ideal gas is a theoretical gas composed of a set of randomly-moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law. At normal conditions such as standard temperature and pressure, most real gases behave qualitatively like an ideal gas. Many gases such as air, nitrogen, oxygen, hydrogen, noble gases, and some heavier gases like carbon dioxide can be treated like ideal gases within reasonable tolerances.
Helium is most likely to behave as an ideal gas when it is under?
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.
Why ammonia doesnt behave as an ideal gas?
Ammonia does not behave as an ideal gas because it experiences intermolecular forces such as hydrogen bonding. These forces cause ammonia molecules to have interactions with each other, leading to deviations from the ideal gas law at high pressures and low temperatures.
What gas conforms to the gas laws at all conditions of temperature and pressure?
An ideal gas conforming to the ideal gas law (PV = nRT) would behave at all conditions of temperature and pressure. However, in reality, no gas perfectly conforms to the gas laws under all conditions.
Why is the boyles law applicable only the idealgases?
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
Under which conditions does a real gas behave most like an ideal gas?
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.
Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
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.
