Question

Question #5aafc

Answer 1

`PV=nRT`

Explanation:

The ideal gas equation is

`PV=nRT`

`P` is the pressure, `V` is the volume, `n` is the amount of moles of substance, `R` is the ideal gas constant, and `T` is the temperature.

Know that the constant `R` varies, because of the different units that can be used to measure `P` and `V` quantities.

For example, `R=0.082 \ L \ atm \ mol^-1 \ K^-1` if and only if `P` is measured in `atm` and `V` is measured in liters, and `T` is measured in Kelvin `(K)`.

Answer 2

It is a combination of several independent relationships, and it is "Ideal" because is assumes "perfect behaviour" of the gases. Ref.: Boyle's Law, Charles' Law, Gay-Lussac's Law and Avogadro's Law. https://en.wikibooks.org/wiki/General_Chemistry/Gas_Laws

Explanation:

The previous answer was technically correct, and can also be found in any textbook. My answer is to explain the title, and the fact that unless gasses are are relatively low pressures and medium temperature ranges the values obtained will be slightly in error from the "real" conditions.

This is important when dealing with some gaseous compounds that are MUCH less than "ideal" in behaviour, and when dealing with gases at extreme temperatures or pressures. Other correction factors need to be applied for accurate assessments in those cases.