If equal weights of oxygen and nitrogen are placed in separate containers of equal volume at the same temperature, which one of the following statements is true?

(mol wt: ${\mathrm{N}}_2=28,{\mathrm{O}}_2=32$)

The ideal gas equation is $\mathrm{PV}=\mathrm{nRT}=\frac{\mathrm{m}}{\mathrm{M}}\mathrm{RT}$

Here,  is the molecular weight and m is the mass.

The volume, mass, and temperature are the same for oxygen and nitrogen.

As a result, the relationship between their pressures and molecular weights is inverse.

Nitrogen's molecular weight (28) is lower than oxygen's (32).

As a result, the nitrogen flask has a higher pressure than the oxygen flask.