a real gas is introduced to a flask of volume v. is the corrected volume of the gas greater or less than V?
Ammonia has a larger a value than neon does. What can you conclude about the relative strength of the attractive forces between molecules of ammonia and between atoms of neon ?
We can conclude that the attraction forces of Ammonia are much stronger than those of Neon. This is because "a" represents the strength of the attractive forces.
Large values of a indicate strong attractive forces.
The corrected volume is less than the available volume.
Volume of real >Volume of ideal
Because we can't ignore the molecular volume of real gases ,but we conclude that;
According to kinetic molecular theory:
The volume of ideal gas is negligible.
Well, introducing a real gas to a flask might make it feel a bit inflated, so I'd say the corrected volume could be greater than V!
As for the relative strength of the attractive forces, if ammonia has a larger a value than neon, we can conclude that the attractive forces between molecules of ammonia are stronger than between atoms of neon. So, ammonia really knows how to pull things together, while neon prefers to do its own thing!
To answer the first question, we need to consider the behavior of a real gas. Unlike an ideal gas, a real gas does not strictly follow the ideal gas law, especially at high pressures or low temperatures. Real gases have intermolecular forces and occupy some volume, unlike ideal gases.
When a real gas is introduced into a flask of volume V, the actual volume occupied by the gas particles will be greater than V due to the intermolecular attractions and the volume occupied by the gas molecules themselves. Therefore, the corrected volume of the gas (which accounts for the intermolecular forces and molecular size) will be greater than the apparent volume V.
Now, let's address the second question about the relative strength of attractive forces between molecules of ammonia and atoms of neon. The "a" value, also known as the van der Waals constant, is a measure of the strength of the intermolecular forces in a real gas. A larger "a" value indicates stronger intermolecular attractions.
Given that ammonia has a larger "a" value than neon, we can conclude that the attractive forces between molecules of ammonia are stronger than the attractive forces between atoms of neon. This is because ammonia molecules have dipole-dipole interactions (due to its polar nature) and hydrogen bonding (if present), whereas neon consists of non-polar atoms and only experiences weaker London dispersion forces.
Therefore, ammonia exhibits stronger intermolecular attractions compared to neon, as indicated by its larger "a" value.