sequence stoichiometry 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: N₂(g) +3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH, (g)+ 20,(g) HNO₂(g) + H₂O(g) 1 Suppose the yield of the first step is 65.% and the yield of the second step is 78.%. 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. 0 0.2 0.² ロ・ロ 0/5 00 8 Allle dla Ar
sequence stoichiometry 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: N₂(g) +3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH, (g)+ 20,(g) HNO₂(g) + H₂O(g) 1 Suppose the yield of the first step is 65.% and the yield of the second step is 78.%. 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. 0 0.2 0.² ロ・ロ 0/5 00 8 Allle dla Ar
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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:
N2(g) +3H2(g) =2NH3(g)
In the second step, ammonia and oxygen react to form, nitric acid (HNO3) and water:
NH3(g) +2O2(g) = HNO3(g) +H2O(g).
Suppose the yield of the first step is 65% in the yield of the second step is 78%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol and is rounded to two significant digits.
![CHEM107 02 2494: ALEKS X A ALEKS-Allie Fleming - Learn X +
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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:
N₂(g) + 3H₂(g) → 2NH₂ (g)
In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water:
NH, (g) + 20₂(g) → HNO₂(g) + H₂O(g)
-
2
O CHEMICAL REACTIONS
Reaction sequence stoichiometry
Suppose the yield of the first step is 65.% and the yield of the second step is 78.%. 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.
0
Explanation
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Transcribed Image Text:CHEM107 02 2494: ALEKS X A ALEKS-Allie Fleming - Learn X +
с www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-lgNslkr7j8P3jH-IQUHIQg6bJxmeSyVpHOEB1plef9xyC5Ca9QIUguxsOh6JaPkoFmRjOsHfBG1fSo7eqF-p1MWN53Co8UxtGsOSWInj4Y-2xq?10Bw7QYj... ✰
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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:
N₂(g) + 3H₂(g) → 2NH₂ (g)
In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water:
NH, (g) + 20₂(g) → HNO₂(g) + H₂O(g)
-
2
O CHEMICAL REACTIONS
Reaction sequence stoichiometry
Suppose the yield of the first step is 65.% and the yield of the second step is 78.%. 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.
0
Explanation
W
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3
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-
$
4
R
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8
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0° 0.0
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6
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B
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7
144
N
*
19 pll
8
J
3
NO DDI
(
9
K
<
O
CELLE
GABAT IDAKUT MAKAN. MAKAN 0/5
L
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© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
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+
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