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. 1.98 g H2 is allowed to react with 10.0 g N2, producing 2.47 g NH3. Part A What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

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

no of moles of H2   = W/G.M.Wt

                              =1.98/2 = 0.99 moles

no of moles of N2   = W/G.M.Wt

                                =10/28   = 0.357 moles

1 mole of N2 react with 3 moles of H2

0.357 moles of N2 react with = 3*0.357/1    = 1.071moles of H2

H2 is limiting reactant

3 moles of H2 react with N2 to gives 2 moles of NH3

0.99 moles of H2 react with N2 to gives = 2*0.99/3 = 0.66 moles of NH3

mass of NH3   = no of moles * gram molar mass

                        = 0.66*17 = 11.22 g

Theoretical yield of NH3   = 11.2g >>>>answer

percent yield   = 2.47*100/11.2   = 22%

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