Le Chatelier's Principle

Mr. Anderson explains Le Chatelier's Principle, which describes how reversible reactions respond to disturbances in equilibrium. He uses examples like the Haber process to illustrate how changes in concentration, pressure, and temperature can shift reactions to re-establish equilibrium. The video also covers strategies to increase yield in chemical reactions by manipulating these factors.

Describe the effect of decreasing volume on the equilibrium of a gas reaction.

How can one increase the percent yield of a reaction according to Le Chatelier's Principle?

In the context of the Haber process, how can increasing reactants affect ammonia production?