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 15.6 grams H2 in the presence of excess N2 gas according to the following balanced chemical equation: N2(g) + 3 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 15.6 grams H2 in the presence of excess N2 gas according to the following balanced chemical equation: N2(g) + 3 H2(g) → 2 NH3(g)
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter11: Stoichiometry
Section: Chapter Questions
Problem 59A
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Question 72 of 91
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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 15.6
grams H2 in the presence of excess N2 gas according to
the following balanced chemical equation:
N2(g) +
H2(g) →
NH3(g)
STARTING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
2.6
28.02
1.01
g/mol H2
5.2
3
7.72
mol H2
0.918
2
2.02
g NH3
0.612
14.01
g/mol NH3
0.306
15.6
mol NH3
1
17.04
g H2
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Transcribed Image Text:4:52 1
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Question 71 of 91
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According to the balanced reaction below, calculate the
moles of NH3 that form when
4.2
mol of N2H4
completely reacts
3
N2H4(1) →
4
NH3(g) + N2(g)
STARTING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
16.8
17.04
g N2
1
mol N2H.
4.2
3.2
mol NH3
g NH3
5.6
mol N2
28.02
g N2H4
6.022 x 1023
32.06
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