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.
I answered this just now at the original; I'm a little late catching up from yesterday.
A is right.
C is right.
B is not right.
If NH3 is REMOVED as it is formed then the reaction must shift to the right in order to replace that which has been removed.
Thanks Bob!
Your answers for (a) and (c) are correct, but there is a slight correction needed in your answer for (b).
(a) Additional nitrogen is added to the system:
When additional nitrogen is added to the system, according to Le Chatelier's principle, the equilibrium will shift in the direction that reduces the concentration of nitrogen. In this case, since nitrogen is a reactant, the system will shift to the right to produce more ammonia. The equilibrium will shift towards the side with fewer moles of gas to reduce the increase in nitrogen concentration.
(b) Ammonia is removed from the system as it forms:
When ammonia is removed from the system, the equilibrium will shift in the direction that replaces the lost ammonia. In this case, ammonia is a product, so the system will shift to the right to produce more ammonia to replenish what was removed. The equilibrium will shift towards the side with fewer moles of gas to increase the ammonia concentration.
(c) The pressure on the system is increased:
When the pressure on the system is increased, according to Le Chatelier's principle, the equilibrium will shift in the direction that reduces the total number of moles of gas. In this case, since there are fewer moles of gas on the product side, the equilibrium will shift to the right to produce more ammonia. The shift towards the side with fewer moles of gas helps in reducing the pressure.
In summary:
(a) Additional nitrogen is added: Shifts right to produce more ammonia.
(b) Ammonia is removed: Shifts right to replace the lost ammonia.
(c) Pressure is increased: Shifts right to reduce the total number of moles of gas.