The van der Waals' equation for a real gas is given by the formula (P+(n2 a/V2))(V-n b)=n R T where P, V, T and n are the pressure, volume, temperature and the number of moles of the gas. Which one is the correct interpretation for the parameter a?

Question

The van der Waals' equation for a real gas is given by the formula (P+(n2 a/V2))(V-n b)=n R T where P, V, T and n are the pressure, volume, temperature and the number of moles of the gas. Which one is the correct interpretation for the parameter a? (A) The parameter a accounts for the finite size of the molecule, riot included temperature in the ideal gas law (B) The parameter a accounts for the shape of gas phase molecules (C) The parameter a accounts for intermolecular interaction's present in the molecule (D) The parameter a has no physical significance and van der Waals? introduced it as a numerical correction factor only

Tardigrade Admin · Accepted Answer

In van der Waals' equation for real gases, a accounts for intermolecular interactions present in the gases.

Q. The van der Waals' equation for a real gas is given by the formula (P+V2n2a​)(V−nb)=nRT where P,V,T and n are the pressure, volume, temperature and the number of moles of the gas. Which one is the correct interpretation for the parameter a?

The parameter a accounts for the finite size of the molecule, riot included temperature in the ideal gas law

The parameter a accounts for the shape of gas phase molecules

The parameter a accounts for intermolecular interaction's present in the molecule

The parameter a has no physical significance and van der Waals? introduced it as a numerical correction factor only

In van der Waals' equation for real gases, a accounts for intermolecular interactions present in the gases.

Q. The van der Waals' equation for a real gas is given by the formula $(P + \frac{n ^{2} a}{V ^{2}}) (V - nb) = n RT$ where $P, V, T$ and $n$ are the pressure, volume, temperature and the number of moles of the gas. Which one is the correct interpretation for the parameter a?