Nitrogen combine with hydrogen to produce ammonia
at a
ratio:

Assuming that the reaction has indeed proceeded to completion- with all nitrogen used up as the question has indicated.
of hydrogen gas would have been consumed while
of ammonia would have been produced. The final mixture would therefore contain
Apply the ideal gas law to find the total pressure inside the container and the respective partial pressure of hydrogen and ammonia:
Additional information
Relative atomic mass(Ar) : A=7, G=16
The empirical formula : A₂G
<h3>Further explanation</h3>
Given
3.5g of element A
4.0g of element G
Required
the empirical formula for this compound
Solution
The empirical formula is the smallest comparison of atoms of compound forming elements.
The empirical formula also shows the simplest mole ratio of the constituent elements of the compound
mol of element A :

mol of element G :

mol ratio A : G = 0.5 : 0.25 = 2 : 1
Methane, CH4, would have the lowest boiling point among the three since it has the lowest number of carbon and has no functional groups. Methanol would have the highest boiling point since it has a functional group which contains hydrogen bonding which much stronger than the one in CH3Cl. Hope this helps.<span />
Yes! You're correct! Hope this helps! :D