The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows. N₂(g) + 3 H₂(g) 2 NH₃(g)
ΔH = -92.2 kJ
Given a system that is initially at equilibrium,which of the following actions cause the reaction to proceed to the left?

Question

The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows. N₂(g) + 3 H₂(g)

The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows. N<sub>2</sub>(g) + 3 H<sub>2</sub>(g) 2 NH<sub>3</sub>(g) ΔH = -92.2 kJ Given a system that is initially at equilibrium,which of the following actions cause the reaction to proceed to the left? A) adding N<sub>2</sub>(g) B) removing NH<sub>3</sub>(g) C) adding a catalyst D) decreasing the temperature E) removing H<sub>2</sub>(g)

2 NH₃(g)
ΔH = -92.2 kJ
Given a system that is initially at equilibrium,which of the following actions cause the reaction to proceed to the left?

Quizplus · Accepted Answer

According to Le Chatelier's principle, removing one of the reactants (in this case, H₂(g)) will shift the equilibrium towards the side with more of that reactant, which is the left side. Therefore, removing H₂(g) will cause the reaction to proceed to the left.

The Thermochemical Equation for the Formation of Ammonia from Elemental