N2(g)+3H2(g) -> 2NH3(g)+ 22000 cal
Consider the reaction is at equilibrium. Explain how the equilibrium is shifted when a. more N is added b. more H is added c. ammonia is removed
Le Chatelier's Principle says, in simple terms, that a system in equilibrium will try to undo what we do to it.
If we add more N it will shift to use N. So it will shift to the right.
If we remove NH3 it will shift to add NH3 back so it will shift to the right.
a) When more N2 gas is added to the reaction, according to Le Chatelier's Principle, the equilibrium will shift to the right to counteract the increase in reactant concentration. This means that more NH3 gas will be produced until a new equilibrium is established.
b) If more H2 gas is added, the equilibrium will again shift to the right to counteract the increase in reactant concentration. This will result in an increase in the production of NH3 gas until a new equilibrium is reached.
c) When ammonia gas (NH3) is removed from the reaction, Le Chatelier's Principle predicts that the equilibrium will shift to the left to compensate for the decrease in product concentration. This will result in the production of N2 and H2 gases until a new equilibrium is achieved.
To understand how the equilibrium of the given reaction is affected by adding or removing reactants or products, we need to analyze the reaction based on Le Chatelier's principle. According to this principle, when a stress is applied to a system at equilibrium, the system will shift in a way that partially offsets the applied stress and restores equilibrium.
a. When more N2 is added:
If more N2 is added to the reaction mixture, the concentration of N2 increases. According to Le Chatelier's principle, the equilibrium will shift to reduce the excessive N2 concentration. To offset the stress of increased N2, the reaction will move in the forward direction (to the right) to consume the excess N2. As a result, more NH3 will be formed, and the reaction will be pushed towards the products.
b. When more H2 is added:
If more H2 is added to the reaction mixture, the concentration of H2 increases. According to Le Chatelier's principle, the equilibrium will shift to reduce the excessive H2 concentration. To offset the stress of increased H2, the reaction will move in the forward direction (to the right) to consume the excess H2. As a result, more NH3 will be formed, and the reaction will be pushed towards the products.
c. When ammonia (NH3) is removed:
If ammonia is removed from the reaction mixture, the concentration of NH3 decreases. According to Le Chatelier's principle, the equilibrium will shift to compensate for the lost NH3. To offset the stress of decreased NH3, the reaction will move in the reverse direction (to the left) to produce more NH3. As a result, the reaction will be pushed towards the reactants.
In summary, by adding more of one of the reactants (N2 or H2), the equilibrium will shift towards the products (NH3). Conversely, by removing one of the products (NH3), the equilibrium will shift towards the reactants (N2 and H2).