Question

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: 2 NH,(8) N2(8) + 3H2(8) In the second step, ammonia and oxygen react to form nitric acid (HNO) and water: NH5()+ 20,(8) HNO,(8) + H,O(8) Suppose the yleld of the first step is 62. % and the yield of the second step is 71.%. Calculate the mass of nitrogen required to make 7.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. ? X

Answer 1

From the balanced reactions I male al HNO is obtained from a mole NH₃ 63g HNO is obtained from 17g NH₃ . 7008 HNO will be ablained from 17x7000 g NH3 = 1888.89 g Nethe We need 1888.89 g NH₃ from first slep suales of Nette is obtained from a mole Na - 34 g NH3 is abtaind from 28 g Na in 1888-898 Ntig will be obtained from 28 x 1888.89 g Na = 1555.56 & Na = ( 106 kg N₂ And. 28