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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: N(g) + 3 H,(g) → 2 NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO,) and water: NH3(g) + 20,(g) → HNO,(g) + H,O(g) Suppose the yield of the first step is 78.% and the yield of the second step is 91.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.

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: N(g) + 3 H,(g) → 2 NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO,) and water: NH3(g) + 20,(g) → HNO,(g) + H,O(g) Suppose the yield of the first step is 78.% and the yield of the second step is 91.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
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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: N(g) + 3 H,(g) → 2 NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO,) and water: NH3(g) + 20,(g) → HNO,(g) + H,O(g) Suppose the yield of the first step is 78.% and the yield of the second step is 91.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.
Transcribed Image Text: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: N(g) + 3 H,(g) → 2 NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO,) and water: NH3(g) + 20,(g) → HNO,(g) + H,O(g) Suppose the yield of the first step is 78.% and the yield of the second step is 91.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.
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