1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 3H₂(g) 2NH3(g) 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 Construct an expression for K and calculate the numerical value of the equilibrium constant, K C N₂ (8) 2 + DH is negative С (ii) At 500°C K = 0.062 mol-2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.

1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 3H₂(g) 2NH3(g) 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 Construct an expression for K and calculate the numerical value of the equilibrium constant, K C N₂ (8) 2 + DH is negative С (ii) At 500°C K = 0.062 mol-2dm. Compare this value to the one you calculated in 3(i) 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

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Similar questions

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