1. We know that higher the Molecular Mass, more is the Van der Wall Forces, thus higher inter molecular forces and hence increased viscosity, in case of liquids. Now, with out getting into the experimental viscosity values of a, b and c, it can be seen that the Molecular Mass increases as:
Benzene < Phenol < Thiophenol
thus the viscosity should increase in the same order at Room Temperture. However,
its not the case. The increasing order viscosity at room temp. is:
Benzene < Thiophenol < Phenol
It is because we also have to consider the hydrogen bonding in case of Phenol.
As the temperature of observation is 50
oC, at this elevated temp. the viscosity of all three will decrease due to thermal agitation. But the H Bonding completely vanishes for phenol. Thus, the new viscosity order would be:
Benzene < Phenol < Thiophenol
2. Again going by the Molecular Mass theory, the order should be:
NH3 < Cl2 < C6H6 < C6H5Cl
However, here also H bonding in NH
3 dominates Molecular Mass of Cl
2. Therefore, the actual order is:
Cl2 < NH3 < C6H6 < C6H5Cl