Question

Consider the following reaction at equilibrium: 2 NH3(g) ⇄ N2(g) + 3 H2(g) What does Le Chatelier's principle predict will happen when adding N2 (g) to the system at equilibrium?

Answer 1

Adding N2 (g) to the reaction at equilibrium will shift the equilibrium toward the reverse reaction to consume the added N2, leading to an increase in NH3 concentration and a slight decrease in N2 and H2 concentrations.

Step-by-step explanation:

When N2 (g) is added to the system at equilibrium for the reaction 2 NH3(g) ⇌ N2(g) + 3 H2(g), Le Chatelier's principle predicts that the system will respond to this change by shifting the equilibrium to counteract the addition. In this case, the system will favor the reverse reaction, which consumes N2 and produces NH3, in order to reduce the concentration of N2 that was added. Over time, the system reaches a new equilibrium where the concentration of NH3 has increased, and the concentrations of N2 and H2 have decreased slightly compared to their levels prior to adding extra N2, while the equilibrium constant (Keq) remains unchanged.

Answer 2

Answer : The equilibrium will shift in the left direction.

Explanation :

Le-Chatelier's principle : This principle states that if any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

The given reaction is:

`2NH_3(g)\rightleftharpoons N_2(g)+3H_2(g)`

As per question, when we are adding
`N_2` then the concentration of
`N_2` is increased on product side then the equilibrium will shift in the direction where decrease of concentration of
`N_2` takes place. Therefore, the equilibrium will shift in the left direction.

Thus, the equilibrium will shift in the left direction.