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.

1.33g H2 is allowed to react with 10.3g N2, producing 3.00g NH3.

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

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

Explanation / Answer

3H2(g)+N2(g)<==>2NH3(g)

6g(H2) + 28g(N2)<==>34g(NH3)...........(1)

6g H2 reacts stiochiometrically with=28g N2

1.33g H2 reacts with=28/6*1.33=6.21gN2 [H2 is limiting and N2 is in excess) so divide eq(1) by 4.51

1.33g(H2) + 6.21g(N2)<==>7.54g(NH3)Theoratical yield

%age yield=actual yield/theoratical yield*100=3.00g/7.54g*100=39.79%

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