Answer:
The equilibrium shifts to the right, shifting towards the products, thereby favouring forward reaction, leading to the production of more product (NH₃) and a reduction in the rate of backward reaction, resulting in a decrease in the production of reactant N₂ in the reaction.
Explanation:
Complete Question
Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:
N₂ (g) + H₂ (g) ⇌ NH₃ (g)
When the concentration of H₂(g) is increased by adding more hydrogen gas to the container at constant temperature, the equilibrium shifts
Solution
Le Chatelier's Principle explains the behaviour of the equilibrium in response to disturbances in properties for chemical reactions.
The principle states that, if the concentration, temperature and/or pressure of a chemical reaction at equilibrium is changed, the equilibrium position shifts to remedy this changes.
So, for a chemical reaction at equilibrium, provided that the other factors such as temperature and pressure remain constant, if more reactants are added (more H₂ is pumped into the reacting container), the equilibrium responds by shifting to the right, shifting towards the products, thereby favouring forward reaction, leading to the production of more product (NH₃) and a reduction in the rate of backward reaction, resulting in a decrease in the production of reactant N₂ in the reaction.
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