The Haber-Bosch process is a very important industrial process. In the Haber-Bos

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

3H2(g)+N2(g)?2NH3(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.

1.33g H2 is allowed to react with 9.55g N2, producing 2.30g NH3.

Part A

What is the theoretical yield for this reaction under the given conditions?

Part B

What is the percent yield for this reaction under the given conditions?

Explanation / Answer

converting to equivallance:

H2 : 0.221 eqv

N2 : 0.341 eqv

so, N2 is excess.

moles of product = 0.221*2 mols = 0.442 mols = 7.514 gm NH3

percent yield = (2.3/7.514)*100% = 30.60%

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