Correct Answer - Option 1 : Gas C will occupy more volume than gas A; gas B will be more compressible than gas D
Concept:
If the values of ‘b’ for two gasses are same but the values of ‘a’ are different, then the gas having a larger value. ‘a’ will occupy lesser volume. Since it will have larger force of attraction and therefore, lesser distance between its molecules.
If values of ‘a’ for two gases are same but the values of ’b’ are different then the smaller value of ‘b’ will occupy lesser volume and, therefore, will be more compressible.
In Vander wall’s equation, a and b are constant. Here ‘a’ is defined as greater the value of ‘a’, greater the force of attraction and smaller is the volume and ‘b’ is defined the greater the value of ' b' higher will be the effective volume & less will be the compressibility. Gas 'C' will occupy more volume than Gas 'A’, Gas 'B' will be more compressible than Gas 'D'.
The van der Waals force, is a distance-dependent interaction between atoms or molecules. Unlike ionic or covalent bonds, these attractions do not result from a chemical electronic bond; they are comparatively weak and therefore more susceptible to disturbance. The van der Waals force quickly vanishes at longer distances between interacting molecules.
So, Gas C will occupy more volume than gas A; gas B will be more compressible than gas D.
