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.

1.14 g H2 is allowed to react with 10.1 g N2, producing 1.47 gNH3.

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.

Part B

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

Answer 1

part A

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

3 mol          1 mol                          2 mol

6 g              28 g                          34 g       ------------ theoritical yield

1.14 g        10.1 g                        1.47        ------------- actual yield

theoritical yield = 34.0 g

Part B :

percent yield = (actual yield / theoritical yield ) x 100

                     = (1.47 / 34 ) x 100

                     = 4.32%