The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows. N₂(g) + 3 H₂(g) $\rightleftharpoons$ 2 NH₃(g)
?H = -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)

\rightleftharpoons

2 NH₃(g)
?H = -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

Removing H₂(g) decreases the concentration of a reactant, causing the equilibrium to shift to the left to produce more H₂(g).

The Thermochemical Equation for the Formation of Ammonia from Elemental ⇌\rightleftharpoons⇌