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13 Dec 2019
The Haber-Bosch process is a very important industrial process.In the Haber-Bosch process, hydrogen gas reacts with nitrogen gasto produce ammonia according to the equation
3H2(g)+N2(g)?2NH3(g)
The ammonia produced in the Haber-Bosch process has a wide rangeof uses, from fertilizer to pharmaceuticals. However, theproduction of ammonia is difficult, resulting in lower yields thanthose predicted from the chemical equation.
1.33g H2 is allowed to react with 10.3g N2, producing 3.00gNH3.
What is the theoretical yield for this reaction under the givenconditions?
What is the percent yield for this reaction under the givenconditions?
The Haber-Bosch process is a very important industrial process.In the Haber-Bosch process, hydrogen gas reacts with nitrogen gasto produce ammonia according to the equation
3H2(g)+N2(g)?2NH3(g)
The ammonia produced in the Haber-Bosch process has a wide rangeof uses, from fertilizer to pharmaceuticals. However, theproduction of ammonia is difficult, resulting in lower yields thanthose predicted from the chemical equation.
1.33g H2 is allowed to react with 10.3g N2, producing 3.00gNH3.
What is the theoretical yield for this reaction under the givenconditions?
What is the percent yield for this reaction under the givenconditions?
Trinidad TremblayLv2
17 Dec 2019
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