NH3 gas is liquefied more easily than N2. Hence,
van der waals' constants a and b of NH3 > that of N2
van der waals' constant a and b of NH3 < that of N2
aNH3>aN2 but bNH3<bN2
aNH3<aN2 but bNH3>bN2
If a gas is liquefied, it means volume is decreased and attractive force exists. a is a measure of attractive force and b the co-volume hence,
aNH3>aN2 and bNH3>bN2