N2(g) +H2 (g) -> 2NH3(g).determine how much NH3 would be produced if 200g of H2 reacts with excess of N2. ?

Question

(ATOMIC WEIGHT OF N=14U,H=1U.)........ plz tell me the answer as soon as possible.

Answer 1

N2(g) +3H2 (g) -> 2NH3(g) Balanced

200g of H2 = 200/2.016=99.206 moles of H2

The eqn suggests that

3 moles of H2 produces 2*17 g NH3

99.206 moles of H2 produces 2*17*99.206/3 g NH3

                                         =1124.3386 g NH3

Answer 2

I know from the Haber's process that the manufacture of ammonia is supposed to be a reversible reaction.

As such it never reaches completion. You can only increase or decrease the concentration of ammonia in the equilibrium mixture (according to Le Chatelier's principle) by varying the conditions.

Optimum conditions as used in the haber's process:

1) a compromise temperature of 400-500 degrees celcius

2) presence of finely powered iron as catalyst

3 a pressure of 250 atmosphere.