ANS:B - > R

For a real gas obeying the Van der Waals equation of state, the difference between the molar specific heat at constant pressure (𝐶𝑝Cp​) and the molar specific heat at constant volume (𝐶𝑣Cv​) is typically less than 𝑅R, the universal gas constant. In the Van der Waals equation, the term (𝐶𝑝−𝐶𝑣)(Cp​−Cv​) represents the difference between the molar specific heats at constant pressure and constant volume, respectively. For a real gas, this difference is generally less than 𝑅R. So, the correct statement is: (𝐶𝑝−𝐶𝑣)<𝑅(Cp​−Cv​)<R