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.

1.10 g H2 is allowed to react with 9.72 g N2, producing 1.68 g NH3.

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? Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

3 H2 + N2 -----------------> 2 NH3

moles of H2 = 1.10 / 2 = 0.550 mol

Moles of N2 = 9.72 / 28 = 0.347 mol

From balanced equation,

3 mol H2 = 1 mol N2

Hence, 0.55 mol H2 = 1*0.55/3 = 0.183 mol

So, H2 is limiting reacgent.

3 mol H2 = 2 mol NH3

Then, 0.55 mol H2 = 2*0.55 /3 = 0.367 mol of NH3

Mass of NH3 = theoretical yield = 0.367 * 17 = 6.24 6.

(b)

% yield = (1.68/6.24) * 100 = 26.9%

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