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Nitrogen reacts with hydrogen in this exothermic reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) Which change increases the equilibrium yield of ammonia but has no effect on the value of the equilibrium constant Kₑ? A Add a catalyst B Increase the partial pressure of nitrogen C Decrease the temperature D Decrease the total pressure - AQA - A-Level Chemistry - Question 12 - 2019 - Paper 3

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Question 12

Nitrogen-reacts-with-hydrogen-in-this-exothermic-reaction--N₂(g)-+-3H₂(g)-⇌-2NH₃(g)--Which-change-increases-the-equilibrium-yield-of-ammonia-but-has-no-effect-on-the-value-of-the-equilibrium-constant-Kₑ?--A--Add-a-catalyst-B--Increase-the-partial-pressure-of-nitrogen-C--Decrease-the-temperature-D--Decrease-the-total-pressure-AQA-A-Level Chemistry-Question 12-2019-Paper 3.png

Nitrogen reacts with hydrogen in this exothermic reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) Which change increases the equilibrium yield of ammonia but has no effect on the... show full transcript

Worked Solution & Example Answer:Nitrogen reacts with hydrogen in this exothermic reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) Which change increases the equilibrium yield of ammonia but has no effect on the value of the equilibrium constant Kₑ? A Add a catalyst B Increase the partial pressure of nitrogen C Decrease the temperature D Decrease the total pressure - AQA - A-Level Chemistry - Question 12 - 2019 - Paper 3

Step 1

Increase the partial pressure of nitrogen

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Answer

Increasing the partial pressure of nitrogen shifts the equilibrium position to the right, favoring the production of ammonia (NH₃) according to Le Chatelier's principle. Importantly, this change does not affect the equilibrium constant (Kₑ) as it is only dependent on temperature. Therefore, the correct choice is to increase the partial pressure of nitrogen.

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