The term that corrects for the attractive forces present in a real gas in the van der Waals equation is

Explain: Why do real gases show deviation from ideal gas behavior?

The van der Waals equation of state for a real gas is given. For $n$ moles of a real gas,the equation can be expressed as:

The compressibility factor for a van der Waal gas at high pressure is

Which of the given sets of temperature and pressure will cause a gas to exhibit the greatest deviation from ideal gas behavior?

For a real gas (molar mass $= 60 \, g/mol$),if the density at the critical point is $0.80 \, g/cm^3$ and its critical temperature $T_c = \frac{4 \times 10^5}{821} \, K$,then the van der Waals constant $a$ (in $atm \, L^2 \, mol^{-2}$) is: