It seems like you're asking about the "a" and "b" values in the van der Waals equation, which describes the behavior of real gases. Here's how to figure out which has a greater value for each:

Understanding the van der Waals Equation

The van der Waals equation is:

[ (P + a(n/V)^2) ] * (V - nb) = nRT

Where:

* P: Pressure

* V: Volume

* n: Number of moles

* R: Ideal gas constant

* T: Temperature

"a" and "b" Values

* "a" (Attraction): This term accounts for the attractive forces between gas molecules. Larger "a" values indicate stronger intermolecular forces.

* "b" (Volume): This term represents the volume occupied by the gas molecules themselves. Larger "b" values indicate larger molecules.

Comparing N2 and NH3

1. "a" Value (Attraction): NH3 will have a larger "a" value than N2. This is because NH3 can participate in hydrogen bonding, a very strong intermolecular force, due to the presence of the polar N-H bond. N2 only has weak London dispersion forces.

2. "b" Value (Volume): NH3 will have a larger "b" value than N2. This is because the NH3 molecule is larger than the N2 molecule.

Conclusion:

* NH3 will have a larger "a" value due to its stronger intermolecular forces.

* NH3 will have a larger "b" value because its molecules are larger.