How many grams of NH3 can be produced form the reaction of 28 g of nitrogen and 25g of hydrogen?

Answer 1

I doubt if N2 and H2 would react to make NH3, however,
because Nitrogen is 28/(28+3) or 90 percent of NH3, so Hydrogen is then 3 percent, it is obvious that most of the mass is in N.
So if you use 28 grams of Nitrogen, you only need a few grams of Hydrogen
grams. If 28 grams is 97 percent, the the hydrogen 3 percent must be...
28/97=x/3 or x= .9 grams, so how much NH3? what is 28+.9*3 ?

Answer 2

At the right temperature and pressure and with a suitable catalyst, this reaction produces NH3 commercially. This is a limiting reagent (LR) problem.
N2 + 3H2 ==> 2NH3
mols N2 = 28 g/28 g/mol = 1 mole. You will need 3 mols H2 and you have well over that (25/2 = 12.5 mols H2 initially) so N2 is the LR.
That will produce 1 mol N2 x (2 mols NH3/1 mol N2) = 2 mols NH3.
g NH3 produced = 2 mols x molar mass NH3 = 34 grams.