Question

2kg Nitrogen reacts with 1 Kg hydrogen ? Calculate the mass of ammonia produced.

Answer 1

The reaction is as follows:

N2  +  3H2 ----> 2 NH3
g          g            g

That means 1 mole of nitrogen and 2 moles of Hydrogen produces 2 moles of ammonium.

Molar mass of the gases:
N2-----14 x2 = 28
H2-----1 x 2 = 2
NH3---- 14 + 3 = 17

Find moles of nitrogen and hydrogen:
moles =mass/molar mass
N=  2/ 28 = 0.07143
H=  1/2 =  0.5
 
Find the number of moles of H2 required for this reaction:

Ratio of N:H is 1:3
Therefore if 1 = 0.07143 (moles of nitrogen required)
               then 3= 0.07143 x 3
                         = 0.2143
Find mass of hydrogen required:

Mass =  moles x molar mass
         = 0.2143 x 2
         = 0.4286kg ....while mass available 1kg

moles of nitrogen required:

Ratio N:H  is 1:3    and moles of Hydrogen is 0.5
 then moles of nitrogen required is 0.5/3 = 0.1667

mass required = 0.1667 x 14
                     = 2.3333kg........hence nitrogen is the limiting factor.

Ratio of N: NH3  =1:2 (meaning for every 1 mole of nitrogen there is 2 moles of ammonium produced)

Therefore moles of NH3 produced will be:
Moles of nitrogen used = 0.07143
Hence moles of ammonium = 0.07143 x 2
                                           = 0.1428
mass of ammonium =  mass x molar mass = 0.1428 x 17

                                     = 2.4276 kg

Answer 2

2.4276is the answer

hope it is helpful to you