plz write out answer like the 2nd photo or similar to it Ans :-メStartingAmouatる2す 10:07Question 1 of 12SubmitConsider the Haber-Bosch process for the synthesis of ammoniafrom its elements. Calculate the theoretical yield in moles NH,from the complete reaction of59.8grams N2 in the presenceof excess H2 gas according to the following balanced chemicalequation:N2(g) +H2(g) →NH3(g)STARTING AMOUNTADD FACTORANSWERRESET*( )17.041.01145g/mol N22.1372.7mol NH34.271g/mol NH328.028.54g N23.52g NH,359.8mol N214.017.04

Since hydrogen gas is present in excess, nitrogen gas is the limiting reagent. One mole of nitrogen…

Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, rom the complete reaction of 59.8 grams N. in the presence of excess H2 gas according to the following balanced chemical equation: N2(g) + H2(g) → 2 NH,(g) 3

Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, rom the complete reaction of 59.8 grams N. in the presence of excess H2 gas according to the following balanced chemical equation: N2(g) + H2(g) → 2 NH,(g) 3

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 84AP

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plz write out answer like the 2nd photo or similar to it

10:07
Question 1 of 12
Submit
Consider the Haber-Bosch process for the synthesis of ammonia
from its elements. Calculate the theoretical yield in moles NH,
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)
STARTING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
17.04
1.01
145
g/mol N2
2.13
72.7
mol NH3
4.27
1
g/mol NH3
28.02
8.54
g N2
3.52
g NH,
3
59.8
mol N2
14.01
7.04

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