Say for example you started off with two containers, both filled with the same amount of N2 and H2 in the same 1:3 ratio.
Now let's assume one container is heated to 200 C and one to 400 C.
The container at 400 C will obviously have the reactants forming products at a faster initial rate so therefore will reach equilibrium in a smaller time span.
However, when both containers have reached equilibrium and you compare the equilibrium compositions, will you notice a greater amount of NH3 in the container at 200 C Or 400 C?
I know this seems like a pretty basic question with an obvious answer.....but i just wanted to clarify (since every chemistry textbook i've read doesn't seem to) that the initial temperatures and other conditions affect the eventual equilibrium composition and that they're not just referring to what changing the conditions at equilibrium will do to the composition.
p.s: the answer i have to this question already: The lower temperature will favour the forward exothermic reaction so therefore the NH3 in the 200 C container will be at a higher amount at equilibrium than in the container at 400 C. However, the container at 400 C will obviously have reached equilibrium faster but the NH3 yield will be smaller.