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

Quizplus · Accepted Answer

According to Le Chatelier's principle, removing one of the products (NH₃(g)) will shift the equilibrium to the right to replace what was removed. However, removing one of the reactants (H₂(g)) will shift the equilibrium to the left to try and replace what was removed. Therefore, choice E is the best choice for causing the reaction to proceed to the left. Choice C, adding a catalyst, would not change the position of the equilibrium, but would increase the rate at which it reaches equilibrium. Choices A and D would shift the equilibrium to the right, and choice B would not significantly affect the equilibrium since there is already an excess of nitrogen present.

The Thermochemical Equation for the Formation of Ammonia from Elemental ~~~~~~~~

The Thermochemical Equation for the Formation of Ammonia from Elemental $~~~~~~~~$