(iii) At 500°C K = 0.062 mol2dm. Compare this value to the one you calculated in 3 (ii) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.
(iii) At 500°C K = 0.062 mol2dm. Compare this value to the one you calculated in 3 (ii) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.
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
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 89AP
Related questions
Question
Question iii
![Predict the position of equilibrium when:
(a) both the temperature and pressure are decreased
(b) the temperature is increased and the pressure is decreased
(ii) Explain the reasoning for using compromise temperature and pressure
in industrial processes
1.3
3 (ii) In the Haber process for the production of ammonia the following
reaction occurs:
N₂(g)
+
3H₂(g)
2NH3(g) DH is negative
If the equilibrium concentrations for all the reactants and products at
600°C are:
[N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³
what is the numerical value of the equilibrium constant,
K?
(iii) At 500°C K = 0.062 mol dm. Compare this value to the one you
calculated in 3(ii) above and state whether the yield of ammonia is greater
at 500°C or 600°C and briefly explain your choice.
1.4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F92456534-2e4c-469d-866d-dc8c0d78d0bc%2F7b13dfb7-de0f-47cc-8aeb-66a75a3a12b8%2F8ycfjpk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Predict the position of equilibrium when:
(a) both the temperature and pressure are decreased
(b) the temperature is increased and the pressure is decreased
(ii) Explain the reasoning for using compromise temperature and pressure
in industrial processes
1.3
3 (ii) In the Haber process for the production of ammonia the following
reaction occurs:
N₂(g)
+
3H₂(g)
2NH3(g) DH is negative
If the equilibrium concentrations for all the reactants and products at
600°C are:
[N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³
what is the numerical value of the equilibrium constant,
K?
(iii) At 500°C K = 0.062 mol dm. Compare this value to the one you
calculated in 3(ii) above and state whether the yield of ammonia is greater
at 500°C or 600°C and briefly explain your choice.
1.4
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