The Haber-Bosch process is a very important industrial process.In the Haber-Bosc

Question

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+N2--->2NH3

The ammonia produced in theHaber-Bosch process has a wide range of uses, from fertilizer topharmaceuticals. However, the production of ammonia is difficult,resulting in lower yields than those predicted from the chemicalequation.

1.68 g H2 isallowed to react with 9.66 g N2, producing 2.46 gNH3.  What is the theoretical yield for this reactionunder the given conditions? What is the percent yield forthis reaction under the given conditions?

Can someone help me withthis problem. Being given three values, I’m unsurewhich is the limiting reactant and how to solve this. Pleasehelp! Thanks.

Explanation / Answer

3H2+N2--->2NH3 1.68 g H2 is allowed to react with 9.66 g N2,producing 2.46 g NH3.  What is the theoretical yieldfor this reaction under the given conditions? What is thepercent yield for this reaction under the given conditions Molar mass of NH3 = 14 + 3 * 1 = 17 g 3 * 2 g of H2 reacts with 14 g of N2 6 g of H2 reacts with 14 g of N2 1.68 g of H2 reacts with Xg of N2 X = ( 1.68 * 14 ) / 6 = 3.92 g of N2 So 9.66 - 3.92 = 5.74 g of N2 is left unreacted which is theexcess reactant 6 g of H2 reacts produces 34 g of NH3 1.68 g of H2 produces Y g of NH3 Y = ( 1.68 * 34 ) / 6    = 9.52 g   which is the theoriticalyield % of yield = ( actual yield / theoritical yield ) * 100                = ( 2.46 / 9.52 ) * 100                = 25.84 %

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