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COMEDK2016ChemistryChemical Equilibrium

In the manufacture of ammonia by the Haber's process, N ₂(g)+3 H ₂(g) 2 NH ₃(g)+92.3 ~kJ , which of the following conditions is unfavourable?

Options

  1. AReducing the temperature
  2. BRemoving ammonia as it is formed
  3. CIncreasing the temperature
  4. DIncreasing the pressure

Correct answer

C. Increasing the temperature

Step-by-step solution

For the following reaction, N ₂+3 H ₂ 2 NH ₃+923 ~kJ (i) Reducing temperature is favourable as it is an exothermic process and shift equilibrium towards right. (ii) Also on removing NH ₃ equilibrium shift towards right according to Le-Chatelier's principle. (iii) n_ g is negative for the process. Increase in pressure, equilibrium towards right. For an exothermic reaction, increasing ten, erature shifts the reaction to reactant side.

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