I just wanted to be sure if my answers make any sense.

Thank you;

For the reaction of ammonia:

N2(g) + 3H2(g) --> 2NH3(g)

suppose equilibrium has been established. Explain how and why the position of equilibrium will shift in response to the following changes:

(a) Additional nitrogen is added to the system
(b) Ammonia is removed from the system as it forms
(c) The pressure on the system is increased

(A) I think it will shift right, because we add more reactant so we need to make more product.

(B) If ammonia is removed it will shift to the left to compensate for that loss

(C) If the pressure is increased then the reaction it will shift right because we have less space, so it shifts to where there's less moles.

A is right.

C is right.
B is not.
If NH3 is REMOVED as it is formed, the reaction must shift to the right to form more NH3 to make up for some of it being removed.

(a) Additional nitrogen is added to the system:

To understand how the position of equilibrium will shift in response to this change, let's consider Le Chatelier's Principle. According to this principle, when a system at equilibrium is subjected to a change, it will adjust in a way that counteracts the effect of that change.

In this case, additional nitrogen is added to the system. Since nitrogen is a reactant in the forward reaction, an increase in its concentration will drive the reaction to the right to consume the excess nitrogen. Consequently, the position of equilibrium will shift to the right.

Your answer is correct! Adding more reactant will shift the equilibrium to the right in order to produce more product.

(b) Ammonia is removed from the system as it forms:
Similarly, based on Le Chatelier's Principle, when ammonia is removed from the system, the reaction will adjust to compensate for the loss. Since the removal of ammonia (a product) decreases its concentration, the system will shift to the left, favoring the formation of more ammonia to replace what is lost.

Your answer is correct! Removing product will shift the equilibrium to the left in order to produce more of the product.

(c) The pressure on the system is increased:
Now, let's examine the effect of increasing the pressure on the system. In this reaction, there is a change in the total number of moles of gas between the reactants and products.

Increasing the pressure will shift the equilibrium to the side with fewer gas moles in order to reduce the pressure. In this case, the reactants have fewer gas moles compared to the products. Thus, the position of equilibrium will shift to the left, favoring the formation of fewer gas moles.

Your answer is incorrect. When the pressure is increased, the position of equilibrium will actually shift to the side with fewer gas moles, which in this case is the left. So, it will shift to the left to reduce the pressure.

To summarize:
(a) Adding nitrogen will shift the equilibrium to the right.
(b) Removing ammonia will shift the equilibrium to the left.
(c) Increasing the pressure will shift the equilibrium to the left.