Question

Consider the following Equilibrium

N2(g) + 3H2(g) ⇔ 2NH3(g) + 92.2 kj
which of the following sets of conditions would maximize the production of ammonia in the reaction? explain.
A) Low pressure and high temperature
B) Low pressure and low temperature
C) High pressure and high temperature
D) high pressure and low temperature

Answer 1

C) High pressure and low temperature

Step-by-step explanation:

Le Chatelier's principle. There are 4 mols of gas on the reactants side and 2 moles of gas on the products, as well as some heat. By Le Chatelier's principle, if you increase the pressure (by presumably decreasing the volume), then equilibrium will push to the side with fewer moles, in this case ammonia. Since heat is on the products side, it works like a product. If you take away a product (decreasing temperature/product), then the reaction will push to ammonia to make up for the loss.