Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 59.8 grams N2 in the presence of excess H2 gas according to the following balanced chemical equation: N2(g) + H2(g) - 2 NH3(g)

Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 59.8 grams N2 in the presence of excess H2 gas according to the following balanced chemical equation: N2(g) + H2(g) - 2 NH3(g)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.19PAE: 4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Consider the Haber-Bosch process for the synthesis of ammonia from its elements.
Calculate the theoretical yield in moles NH3 from the complete reaction of 59.8
grams N2 in the presence of excess H2 gas according to the following balanced
chemical equation:
N2(g) +
H2(g) →
NH3(g)
X
TING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
17.04
3.52
1.01
14.01
59.8
3
4.27
8.54
72.7
2.13
28.02
145
1
7.04
g/mol N2
g N2
g/mol NH3
mol NH3
mol N2
g NH3

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