chem 1

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Jarriette kenn D Patenio
Jaymar patana
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Do all ideal gases have the same molar volume?
An ideal gas has the following equation of state (an equation which relates various thermodynamic properties for a substance, such as pressure, temperature and molar volume):

Pv = RT

P - pressure v - molar volume
R - universal gas constant
T - absolute temperature

Clearly the molar volume depends on temperature and pressure, so if two gases are at different conditions then they may have different molar volumes. However, if we assume that both gases are at the same pressure and temperature then they will always have the same molar volume.
How do real gases deviate from the ideal gas?
Ideal gas is only a term used to represent when we are assuming the behavior of a gas fits the principles of an ideal gas, so in reality all gases are real gases and when we use the term ideal gas when we are doing calculations . The difference between the two is that when looking at ideal gases the equations used assume that 1) gases occupy a negligible fraction of the total amount of gas and 2) The interaction between the individual gas molecules with each other is negligible. These two assumptions cause a difference between real and ideal gases, since gases in real life do in fact take up space and have intermolecular interaction.
A chemical bond is an attraction between atoms. This attraction may be seen as the result of different behaviors of the outermost electrons of atoms. Although all of these behaviors merge into each other seamlessly in various bonding situations so that there is no clear line to be drawn between them, nevertheless behaviors of atoms become so qualitatively different as the character of the bond changes quantitatively, that it remains useful and customary to differentiate between the bonds that cause these different properties of condensed matter.
In the simplest view of a so-called 'covalent' bond, one or more electrons (often a pair

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