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 The ammonia produced in the Haber-Bosch process has a wide range of users, from Fortier to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. g H_2 is allowed to react with 10.4 g N_2, producing 1.55 g NH_3. 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

Balanced equation:
3 H2 + N2 = 2 NH3

1.11 gm of H2 = 1.1 / 2.015 = 0.5506 Moles

10.4 gm of N2 = 10.4 /28.01 = 0.3712 Moles

3 Moles of H2 is need to react with one mole of N2 which gives 2 Moles of product (NH3)

Hence according to the H2 is limitng reagent.1.11 Moles of H2 will react with 0.18354 Moles of N2 to produce 0.3670 Moles of NH3

PART A

Theoretical yield = 0.3670 x 17 = 6.251 gm

PART B

Percentage yield = 1.55 x 100 / 6.251 = 24.79 %

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