Can this equation be used to approximate real gases?

Question

PV=nRT and if so is it only an approximate or can actual results be obtained?

Answer 1

Quite in theory, it does not hold for real gases, it is a very good approximation in all day life.

It does not hold only for very high pressure

Answer 2

accurate at low pressure (so that size of particles is negligible to volume of container) and high temperature (overcome the KE and intermolecular forices of attraction b/w molecules).

units of...

P = Pa. 1 atm = 1.01x10^5 Pa

V= m^3. 1 dm^3 = 10^-6 cm^3

n = mol

R = 8.31

T = K. Add 273 to deg C to get T in K

Answer 3

Actually, the ideal gas equation (PV=nRT) works quite well for all gases at low pressures (in the neighborhood of atmospheric pressure) and at temperatures around room temperature.

Oh yes.  Again, depending on the pressure of the gas, it will give good agreement between actual results and calculated results.

At higher pressures (smaller volumes) and lower temperatures the van der Waals equation will give a better prediction of the pressure of a real gas.

Answer 4

it is not used for very high pressure & very low temperature

for these conditons Van Der Waal's eqn. is used

Answer 5

This equation can be used to approximate real gases, and I think that actual results can be obtained in all instances in which the gas laws apply to real gases (i.e. only in instances such as extremely high pressure, exceptionally low temperature etc. will it not necessarily be perfectly accurate).