Knowledge in Gaseous States
Gaseous States (All Formulas and Definitions)
The state of matter distinguished from the solid and liquid states by: relatively low density and viscosity; relatively great expansion and contraction with changes in pressure and temperature; the ability to diffuse readily; and the spontaneous tendency to become distributed uniformly throughout any container. - gas.
Rishi Soni
Vanderwaal equation for real gas
The van der Waals equation is written like this: (P + an2/V2)(V-nb) = nRT. It looks very similar to the ideal gas law (PV = nRT), except now we account for the attraction between the gas molecules with a, and the volume of those molecules with b.The van der Waals equation (or van der Waals equation of state; named after Johannes Diderik van der Waals) is an equation of state that generalizes the ideal gas law based on plausible reasons that real gases do not act ideally. The ideal gas law treats gas molecules as point particles that interact with their containers but not each other, meaning they neither take up space nor change kinetic energy during collisions.[1] The ideal gas law states that volume (V) occupied by n moles of any gas has a pressure (P) at temperature (T) in kelvins given by the following relationship, where R is the gas constant: PV = nRT To account for the volume that a real gas molecule takes up, the van der Waals equation replaces V in the ideal gas law with {\displaystyle (V_{m}-b)}{\displaystyle (V_{m}-b)}, where Vm is the molar volume of the gas and b is the volume that is occupied by one mole of the molecules. This leads to:[1] {\displaystyle P(V_{m}-b)=RT}{\displaystyle P(V_{m}-b)=RT} The second modification made to the ideal gas law accounts for the fact that gas molecules do in fact interact with each other (they usually experience attraction at low pressures and repulsion at high pressures) and that real gases therefore show different compressibility than ideal gases. Van der Waals provided for intermolecular interaction by adding to the observed pressure P in the equation of state a term {\displaystyle a/V_{m}^{2}}{\displaystyle a/V_{m}^{2}}, where a is a constant whose value depends on the gas. The van der Waals equation is therefore written as:[1] {\displaystyle \left(P+a{\frac {1}{V_{m}^{2}}}\right)(V_{m}-b)=RT}{\displaystyle \left(P+a{\frac {1}{V_{m}^{2}}}\right)(V_{m}-b)=RT} and can also be written as the equation below {\displaystyle \left(P+a{\frac {n^{2}}{V^{2}}}\right)(V-nb)=nRT}{\displaystyle \left(P+a{\frac {n^{2}}{V^{2}}}\right)(V-nb)=nRT} where Vm is the molar volume of the gas, R is the universal gas constant, T is temperature, P is pressure, and V is volume. When the molar volume Vm is large, b becomes negligible in comparison with Vm, a/Vm2 becomes negligible with respect to P, and the van der Waals equation reduces to the ideal gas law, PVm=RT.[1]
Akansha pandey
Gaseous State
CBSE Class 12 Detailed notes of chemistry chapter gaseous state Useful for board examination, revision and for other competitive exams
Ishika Sethi