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 pressurein industrial processes1.33 (ii) In the Haber process for the production of ammonia the followingreaction occurs:N₂(g)+3H₂(g)2NH3(g) DH is negativeIf the equilibrium concentrations for all the reactants and products at600°C are:[N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³what is the numerical value of the equilibrium constant,K?(iii) At 500°C K = 0.062 mol dm. Compare this value to the one youcalculated in 3(ii) above and state whether the yield of ammonia is greaterat 500°C or 600°C and briefly explain your choice.1.4

The equilibrium constant of a reaction is determined by dividing the product's concentration by the…

Answered: (iii) At 500°C K = 0.062 mol2dm.…

(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.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter5: Introduction To Chemical Equilibrium

Section: Chapter Questions

Problem 5.16E: 5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of...

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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

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