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Would a gas whose molecules were true geometric points obey the ideal gas law?
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
Why do gases failed to obey ideal gas equation at high temperature and low pressure?
At high temperatures, gas molecules have higher kinetic energy and move faster, leading to increased intermolecular interactions that deviate from ideal behavior. At low pressures, gas molecules are farther apart, reducing the frequency of collisions and interactions among molecules. These factors cause the ideal gas law to break down under these conditions.
What characteristics would make a gas non-ideal?
The gas molecules interact with one another
Is steam considered an ideal gas?
No, steam is not considered an ideal gas. Ideal gases follow the ideal gas law, which assumes that gas particles have no volume and do not interact with each other. Steam, on the other hand, consists of water vapor molecules that have volume and can interact with each other.
Would a gas whose molecules were true geometric points obey the ideal gas law?
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
Why Real gases do not obey gas laws?
Real gases do not obey gas laws because these gases contains forces of attractions among the molecules..and the gases which do not contain forces of attraction among their molecules are called ideal gases and they obey gas laws.
What aspects are not accounted for in the ideal gas law?
The ideal gas law does not account for the volume occupied by gas particles and the interactions between gas molecules.
Why do gases failed to obey ideal gas equation at high temperature and low pressure?
At high temperatures, gas molecules have higher kinetic energy and move faster, leading to increased intermolecular interactions that deviate from ideal behavior. At low pressures, gas molecules are farther apart, reducing the frequency of collisions and interactions among molecules. These factors cause the ideal gas law to break down under these conditions.
Why does gases obey the gas law only in high temperature only?
The ideal gas law effectively treats atoms as point masses that have no interactions except for collisions (no attraction or repulsion). Molecules in hot gasses generally are so far apart that their volume relative to the overall volume is insignificant. They don't attract or repel each other much either at high temperatures because they are mostly too far apart - and - they are moving so quickly that even when close, they are not close for long. As gases cool, the molecules group closer together and move slower and quit behaving in a manner that the ideal gas law can be said to represent well.
What characteristics would make a gas non-ideal?
The gas molecules interact with one another
What is the name of law given to number of molecule is inversely proportional to pressure?
There is no such law. The Ideal Gas Law states that pressure is proportional to the number of molecules Pressure x Volume = number x Ideal gas constant x Temperature
Is steam considered an ideal gas?
No, steam is not considered an ideal gas. Ideal gases follow the ideal gas law, which assumes that gas particles have no volume and do not interact with each other. Steam, on the other hand, consists of water vapor molecules that have volume and can interact with each other.
Is the pressure exerted by gas a result of the ideal gas law?
Yes, the pressure exerted by a gas is a result of the ideal gas law, which describes the relationship between pressure, volume, temperature, and amount of gas molecules. The formula PV = nRT represents the ideal gas law, where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant, and T is temperature.
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.
How did the ideal gas law contribute to the gas law?
All gas laws are absolutely accurate only for an ideal gas.
What are the characteristics of an ideal gas?
1. Elastic Collision (no loss of kinetic energy when molecules hit) 2. Constant, rapid, and random motion 3. No attraction or repulsion between molecules (electromagnetic forces don't effect the collisions)
