Question

2. The Haber process is an industrially important reaction in the production of ammonia (NH, mol mass 17.03 /mol) which is used as a feedstock for the synthesis of nitrogen based fertilizers and explosives. The process involves the direct reaction of nitrogen gas with hydrogen gas to produce ammonia Write a balanced chemical reaction for the above reaction. b) A 500.0 mL reaction vessel was filled with 15.8 g of nitrogen gas are reacted with 11.4 g of hydrogen S. The mixture was heated to 400" for 20 hours. Determine the theoretical yield in grams of ammonin for this reaction c) How many grams of hydrogen gas remain at the end of the reaction?

Answer 1

2 @ Na + 3 H2 - 2NH3 © No. + N₂ + 3H₂ → 2NH3 0.564 mol 5.7mol Mole of NH3 = 2x Mole of Ne 1. i 2x0.564 mol i 1.12857 mol Mass of NH3 = 17.03g/mol x 1.12857 mos = (19.2 g C Mole of H₂ reacted = 3x Mole of M2 = 3x0.564 mos 2 1.692 mol Mole of H₂ gas remain = 15.7 -1.692) mol 34.008 mol Mass of H₂ gas = 4.00842 = 8.016 g 218.02 g)