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)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. 1.86 g H2 is allowed to react with 9.73 g N2, producing 2.16 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
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)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. 1.86 g H2 is allowed to react with 9.73 g N2, producing 2.16 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
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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)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.
1.86 g H2 is allowed to react with 9.73 g N2, producing 2.16 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
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