Question

The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation: 3 H2 (g) + N2 (g) → 2 NH3 (g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. What is the maximum theoretical yield in grams if 1.51 g H2 is allowed to react with 10.1 g N2?

Answer 1

N2 + 3H2   ---> 2NH3

number of moles of H2 = mass/molar mass
= (1.51) / (2)
=0.755 mol

number of moles of N2 = mass/molar mass
= (10.1) / (17)
=0.629 mol

1 mol of N2 requires 3 moles of H2, So clearly H2 is the limiting reagent

from above reaction,
moles of NH3 formed= (2/3)*moles of H2
=(2/3)*0.755 mol
=0.503 mol

mass of NH3 = number of moles * molar mass
                           = 0.503 mol * 17 g/mol
                           = 8.56 g

Answer: 8.56 g