Question

Match the action to the effect on the equilibrium position for the reaction:

N2(g) + 3H2(g) ⇌ 2NH3(g).

Match Term Definition
Removing ammonia A) Shift to the right
Removing hydrogen gas B) No effect
Adding a catalyst C) Shift to the left

Answer 1

Removing ammonia - A) Shift to the right

Removing hydrogen gas - C) Shift to the left

Adding a catalyst - B) No effect

Step-by-step explanation:

Le Chatelier's principle describes the consequences of a system at equilibrium undergoing a change in condition. It states that when a system at equilibrium is disturbed, the system will shift to counteract the change and revert to a state of equilibrium. There are three factors that influence a system's equilibrium: temperature, pressure, and concentration.

In this problem, the factor involved is concentration. The simplest way to understand this is that if the system experiences an increase in the concentration of a reactant, it must shift to the side that favors the products. Conversely, if there is an increase in the concentration of a product, the system will shift to the side that favors production of more reactants.

• Removing ammonia - Ammonia, or NH3, is the product in this reversible reaction. If the concentration of ammonia decreases, the system will shift to produce more of it, so it shifts to the right.
• Removing hydrogen gas - Following the same concept, the decrease in concentration of H2 gas (a reactant) will result in the system shifting to the left to make up for the loss.
• Adding a catalyst - The role of a catalyst is to facilitate a reaction by lowering the activation energy. Le Chatelier's principle does not apply to the addition of a catalyst, and it will have no effect on the position of equilibrium.