The Haber-Botch process is a very important industrial process. In the Haber-Bos

Question

The Haber-Botch 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 3H_2 (g) + N_2 (g) rightarrow 2NH_3(g) The ammonia produced in the Haber-Botch process hat 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. 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. What is the percent yield for this reaction under the given condition? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

mol of H2= mass/MW = 2/2 = 1 mol

mol of N2 = mass/MW = 10.4/28 = 0.371428 mol N2

mol NH3 = 1.18 /17 = 0.06941 mol of NH3

then

theoretical yeld

identify limitin greactant

1 mol of H2 --> 1/3 = 0.333 mol of N2; which we DO have, so H2 is limiting

1 mol of H2 --> 2/3 = 0.66 mol of NH3

mass = mol*MW = 0.66*17 = 11.22 g of NH3

b)

%yield = real/theoretical * 100 = 1.18/11.22 = 0.1051 fractional ---<> = 10.51 %

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