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.

1.21g H2 is allowed to react with 9.56g N2, producing 2.52g 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?

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.

1.21g H2 is allowed to react with 9.56g N2, producing 2.52g 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?

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