Question

In 1909 Fritz Haber discovered the workable conditions under which nitrogen, N2(g), and hydrogen, H2(g), would combine using to produce ammonia. The conditions included
medium temperature (~500oC), very high pressure (~351kPa), and an iron catalyst. The reaction is represented by the equation:
N2(g) + 3H2(g) → 2NH3(g)
How many grams of N2 are required to produce 240.0g NH3?
A) 17.1g N2
B) 120.0g N2
C) 197.7g N2
D) 291.4g N2

Answer 1

Answer:

b is the answer of this question

Answer 2

Balanced equation:  N2 + 3H2 => 2NH3

Moles of NH3 in 240.0 g NH3 : 240.0 g x 1 mol/17 g = 14.1 moles

Moles of N2 needed : 14.1 moles NH3 x 1 mole N2/2 moles NH3

= 7.05 moles N2 needed  

Grams of N2 needed : 7.05 moles x 28 g/mole = 197.4 grams needed