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 uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation 1.83 8 H2 is allowed to react with 9.60g N2. producing 1.97 NH2. 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

From the balanced equation it is observed that 3 mole hydrogen produces 2 mole ammonia.

So, 3 g of hydrogen produces 34 g of ammonia

So, 1.83 g of H2 will produce = 20.74 g ammonia

14 g of nitrogen produces 34g of ammonia.

9.60 of nitrogen produces 23.31 g of ammonia

So, % of yeild = (1.97g/ 20.70g) X 100= 9.52 %

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