How does adding NH3 to the reaction below affect the equilibrium of the reaction?

Question

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

A. Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.

B. Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.

C. Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.

D. Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.

I think the answer is C. Someone please help me.

Answer 1

Le Chatelier's Principle says, when a system in equilibrium is subjected to a stress, the reaction will shift in such as way so as to reduce the stress. In my words it goes like this. When we do something to a system in equilibrium, the system will try to undo what we did. In this question, the answers include both Q and which direction the reactions shifts and we must get both right to get the problem right.
So N2 + 3H2 ==> 2NH3. So add NH3. That means the reaction will try to UNDO the addition of NH3. How can it do that? It will shift to the left so as to decrease the NH3. Of course N2 and H2 will increase. What about Q?
K = (NH3)^2/(N2)(H2)^3 = some number.
So making NH3 larger will make Q larger so Q>K and the reaction will shift to the left.
Your answer of C CAN'T be right. You're increasing NH3 and the reaction must try to get rid of it so it CAN'T try to add NH3 and go forward. Do you get it? If not, what do you not understand.

Answer 2

So A?

Answer 3

The answers is A.